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The Implications of a Solution with a OH- of 4.0 x 10⁻⁵: Navigating the Industrial Landscape
By Dr. Anya Sharma, Ph.D. in Chemical Engineering, Senior Research Scientist at ChemTech Innovations
Published by Industrial Chemistry Insights, a leading publication in the field of applied chemistry and process engineering. Edited by Dr. Ben Carter, Ph.D. in Chemistry, with over 15 years of experience in peer review and technical editing.
Abstract: This article explores the significance of a solution possessing a hydroxide ion (OH⁻) concentration of 4.0 x 10⁻⁵ M. We delve into the implications of this specific concentration across various industries, discussing its impact on material compatibility, process optimization, and environmental considerations. The article also addresses the practical challenges and solutions associated with managing solutions of this nature.
Keywords: a solution has a oh- 4.0x10-5, hydroxide ion concentration, pH, alkalinity, industrial applications, chemical processing, environmental impact, material compatibility.
Understanding the Significance of a Solution with a OH- of 4.0 x 10⁻⁵
The statement "a solution has a OH⁻ of 4.0 x 10⁻⁵" immediately provides crucial information about the solution's chemical properties. This value represents the concentration of hydroxide ions (OH⁻) in moles per liter (M). A hydroxide ion concentration of 4.0 x 10⁻⁵ M indicates a mildly alkaline solution. This seemingly small number has significant ramifications in numerous industrial contexts.
Calculating pH and Implications for Industrial Processes
To fully understand the implications, it's crucial to calculate the pH of the solution. Using the relationship Kw = [H⁺][OH⁻] = 1.0 x 10⁻¹⁴ at 25°C, where Kw is the ion product constant of water, we can determine the hydrogen ion concentration ([H⁺]). Therefore:
[H⁺] = Kw / [OH⁻] = (1.0 x 10⁻¹⁴) / (4.0 x 10⁻⁵) = 2.5 x 10⁻¹⁰ M
This translates to a pH of approximately 9.6. A pH of 9.6 signifies a slightly alkaline environment. This level of alkalinity can significantly influence various industrial processes, impacting both efficiency and safety.
Industrial Applications and Challenges: Where a Solution with a OH- of 4.0 x 10⁻⁵ Matters
1. Chemical Processing: In chemical processing, the alkalinity of a solution dictates reaction rates, product stability, and the compatibility of materials used in processing equipment. A solution with a OH⁻ of 4.0 x 10⁻⁵ might require specific materials to prevent corrosion. For example, certain metals could corrode in this slightly alkaline environment. Selecting appropriate materials like stainless steel or specific polymers becomes crucial.
2. Wastewater Treatment: Wastewater often requires pH adjustments to meet regulatory standards before discharge. A solution with a OH⁻ of 4.0 x 10⁻⁵ might necessitate further treatment or neutralization to achieve the required pH for safe disposal.
3. Pharmaceutical Manufacturing: Many pharmaceutical processes are highly sensitive to pH. Controlling the alkalinity of solutions, such as those used in drug formulation or cleaning validation, is essential to ensure product quality and stability. A solution with a OH⁻ of 4.0 x 10⁻⁵ could necessitate careful control during the manufacturing process.
4. Food and Beverage Industry: pH plays a crucial role in food preservation and quality. The alkalinity of a solution with a OH⁻ of 4.0 x 10⁻⁵ could impact food processing, impacting taste, texture, and shelf life.
5. Environmental Monitoring: Accurate pH measurements are crucial in environmental monitoring, particularly for assessing water quality. Understanding the implications of a solution with a OH⁻ of 4.0 x 10⁻⁵ is vital for interpreting environmental data and implementing effective remediation strategies.
Managing Solutions with a OH- of 4.0 x 10⁻⁵: Safety and Practical Considerations
Handling alkaline solutions requires careful attention to safety protocols. Appropriate personal protective equipment (PPE), including gloves, eye protection, and lab coats, is crucial. Furthermore, adequate ventilation should be ensured to mitigate any potential inhalation hazards. Neutralization procedures should be planned in case of spills or accidental exposure.
Advanced Techniques for Precise pH Control
Maintaining the precise OH⁻ concentration (and thus pH) in industrial processes often requires sophisticated control systems. This could involve the use of automated titrators, pH meters with continuous monitoring capabilities, and feedback control loops that adjust the addition of acids or bases to maintain the desired pH.
Conclusion
The seemingly simple statement, "a solution has a OH⁻ of 4.0 x 10⁻⁵," encapsulates significant information with broad implications across various industries. Understanding the pH and alkalinity associated with this concentration is crucial for optimizing industrial processes, ensuring material compatibility, and maintaining safety standards. Careful consideration of potential hazards and appropriate handling procedures are paramount when working with such solutions.
FAQs
1. How do I convert OH⁻ concentration to pOH? pOH = -log₁₀[OH⁻]. In this case, pOH = -log₁₀(4.0 x 10⁻⁵) ≈ 4.4.
2. What are the potential health hazards associated with handling solutions with high OH⁻ concentrations? High OH⁻ concentrations can cause skin burns, eye irritation, and respiratory problems. Always wear appropriate PPE.
3. How can I neutralize a solution with a high OH⁻ concentration? Slowly add a dilute acid, such as hydrochloric acid (HCl), while constantly monitoring the pH.
4. What are some common industrial uses of alkaline solutions? Alkaline solutions are used in cleaning, wastewater treatment, chemical synthesis, and various manufacturing processes.
5. How does temperature affect the OH⁻ concentration? The ion product constant (Kw) of water is temperature-dependent. Higher temperatures increase Kw, affecting the relationship between [H⁺] and [OH⁻].
6. What are the environmental regulations concerning the discharge of alkaline solutions? Regulations vary depending on location and the specific industry. Compliance with local environmental standards is essential.
7. What types of sensors are used to measure OH⁻ concentration? pH meters are commonly used, indirectly measuring OH⁻ concentration via the relationship with H⁺. Specific ion electrodes can also directly measure OH⁻ concentration.
8. How does the presence of other ions in a solution affect the pH measurement? Other ions can influence the ionic strength of the solution, potentially affecting the accuracy of pH measurements. Ionic strength corrections might be necessary for precise measurements.
9. Can a solution be simultaneously acidic and basic? No, a solution cannot be simultaneously acidic and basic. However, it is possible for a solution to have both acidic and basic components, which can lead to the overall pH of the solution being neutral or close to neutral.
Related Articles
1. The Role of pH in Industrial Wastewater Treatment: This article details the importance of pH control in wastewater treatment processes, focusing on different techniques and regulatory compliance.
2. Material Selection for Alkaline Environments: This piece explores various materials suitable for constructing equipment that handles alkaline solutions, emphasizing corrosion resistance and longevity.
3. Safety Protocols for Handling Alkaline Solutions: A comprehensive guide outlining safety procedures, PPE requirements, and emergency response plans for working with alkaline solutions.
4. pH Control in Pharmaceutical Manufacturing: This article discusses the critical role of pH control in pharmaceutical processes, focusing on maintaining product quality and stability.
5. Advanced pH Measurement Techniques: An exploration of modern pH measurement technologies, including advanced sensor designs and data analysis methods.
6. The Impact of Alkalinity on Environmental Water Quality: This article analyzes the effects of alkaline solutions on aquatic ecosystems and the implications for environmental protection.
7. Corrosion Mechanisms in Alkaline Environments: A detailed study of the corrosion processes that occur when certain materials are exposed to alkaline solutions.
8. Neutralization Reactions and Their Applications: This article examines the principles of neutralization reactions and their practical applications in various industries.
9. Automated pH Control Systems in Chemical Processes: This piece explores the design and implementation of automated systems for precise pH control in chemical manufacturing.
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CHM 2046 Answer Key – Practice Quiz 2 - University of Florida
2O (l) ⇌ CH3COOH (aq) + OH-(aq) b) (2 points) Complete the expression for the base-ionization constant (K b) for CH 3COO-. K b = [CH COO ] [CH COOH][OH ]-3-3. c) (5 points) Calculate …
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A Solution Has A Oh 40x10 5 - x-plane.com
The statement "a solution has a OH⁻ of 4.0 x 10⁻⁵" immediately provides crucial information about the solution's chemical properties. This value represents the concentration of hydroxide ions …
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Week 9 - Solutions Weak Acid and Base Equilibria - umb.edu
Find the concentrations of all species and pH for a 1.0 × 10. 3 M HF solution. 4 + – 10 . You will need to find values for [HF], [H O ], [F ], and [OH ]. This is not acceptable. Notice that C. are …
Tutorial 4 SOLUTION STOICHIOMETRY - Eastern Illinois …
Solution stoichiometry calculations involve chemical reactions taking place in solution. Chemical reactions are written in terms of moles of reactants and products; this molarity concentration …
A Solution Has A Oh 40x10 5 Full PDF - x-plane.com
A Solution Has A Oh 40x10 5: Survival Guide to General Chemistry Patrick E. McMahon,Rosemary McMahon,Bohdan Khomtchouk,2019-02-13 This work evolved over thirty …
Calculating pH, pOH, and [OH - Mr. Arthur's Science Page
A solution is made by dissolving 0.45 mol of sodium hydroxide, NaOH(s), in enough water to make 3.75 L of solution. Determine the pH and pOH of this solution at 25 °C.
CHM 2046 Quiz 2A - Answer Key Spring, 2017 - University of …
Identify each compound as the stronger acid, the stronger base, the weaker acid, or the weaker base. HSO3 - (aq) + H2CO3 (aq) ⇌ HCO3 - (aq) + H2SO3 (aq) d) (2 points) Which one of the …
A Solution Has A Oh 40x10 5 Copy - x-plane.com
The statement "a solution has a OH⁻ of 4.0 x 10⁻⁵" immediately provides crucial information about the solution's chemical properties. This value represents the concentration of hydroxide ions …
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Chemistry 20 - Unit 2 - pH and pOH Notes
a) A solution of acetic acid has a hydronium ion concentration of 0.016 M. b) A bottle of household bleach has a hydronium ion concentration of 1.0 x 10 - 13 M. 2) Calculate the pOH of each of …
CHEM1002 2008-N-5 November 2008 - The University of …
CHEM1002 2008-N-5 November 2008 • Calculate the pH of a 0.020 M solution of Ba(OH) 2. Marks 1 Ba(OH) 2 is a strong base so it will completely dissociate in solution: Ba(OH) 2(s) ! Ba …
Chapter 19 WS Name: - Mr. Miller's Classes
COOH) is 6.40x10-5, what would be the concentration of hydrogen ion in a 0.300 M solution of ethanoic acid? a. Write the equation for the dissociation of ethanoic acid: 𝐻3 𝐻↔ 𝐻3 −+𝐻+ b. …
Chapter 19 WS Name: - Mr. Miller's Classes
COOH) is 6.40x10-5, what would be the concentration of hydrogen ion in a 0.300 M solution of ethanoic acid? a. Write the equation for the dissociation of ethanoic acid: b. Calculate the …
Section 19.1. Acid-Base Buffer Solutions - University of Florida
Problem: Use HF (aq) ⇌ H+(aq) + F-(aq) ? or F-(aq) + H2O (l) ⇌ HF (aq) + OH-(aq) ? Answer: Since both include HF, F-, H+, OH- (the last two are related by [H+][OH-] = 1 x 10-14), we can …
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CH 302 Worksheet 8: Solution Chemistry 1 128 g CH OH x 1 …
(b) Calculate the mole fractions of heptane and octane in the vapor that is in equilibrium with this solution. Xheptane = Pheptane = 18.4 torr = 0.426; Xoctane= Poctane = 24.8 torr = 0.574 Ptotal …
Period Date / / 17 Acid-Base Equilibrium - chemmybear.com
(a) What volume of 0.400-molar NaOH is required to neutralize completely a 5.00 x 10-3 mole sample of pure oxalic acid? (b) Give the equations representing the first and second …
inclass exercise ch16 key - University of North Georgia
8.03 10 ck assumption: 100% 0.005% 5% 0.15 assumption is therefore valid 0.15 ; 8.03 10 14 log 8. b xx K x xM CHNH M CHNH OH M pH OH 90 4. Calculate the pH of 0.020 M solution of NaNO3 …
CHEM1612 Answers to Problem Sheet 6 1. (a) 0.2 M acetic acid
N N NH 3 COO H H N N NH 3 COO H acid conjugatebase (c) As pH = 9.15 is higher than their pK a values, the α-COOH and imidazole N-H groups will exist predominately in their conjugate base …
2021-05-06 06:41 - Mrs. Higgins' Science Pages
19. A solution containing HCI and the weak acid HC102 has of 2.4. Enough KOH(aq) is added to the solution to increase the pH to 105. The amount of which of the following SIEcies increases as the …
Cerritos College - Enroll today for fall 2024 semester classes!
5) For the reaction: 2 N02 02 (g) 2 (g) at923øC , Kcis42.5. oare mixed in a 1.00 liter container at 923 C.in what direction will the reaction your calculation to prove tnat your answer is not a …
pH and pOH Calculations - Brinkster
3) Determine the pH of a 4.3 x 10-4 M NaOH solution. 4) If a solution is created by adding water to 2.3 x 10-4 moles of NaOH and 4.5 x 10-6 moles of HBr until the final volume is 1 L, what is the pH …
Multiple Choice Questions Unit ( ) Chem-100 - Victor Valley …
A 5.00 mL sample of solution has 2.8 x 10-4 g of calcium ions. The ppm concentration is A. 18 ppm B. 56 ppm C. 2.8 x 10-1 ppm D. 2.8 x 10 2 ppm 5. How many mL of 2.50% (m/v) salt solution …
UNIT (5) SOLUTIONS solution - Victor Valley College
5-1 UNIT (5) SOLUTIONS A solution is a homogeneous mixture of two or more substances. 5.1 Solution Terminology Solute and Solvent A simple solution has two components, a solute, and a …
General Chemistry II Jasperse Buffers/Titrations/Solubility.
a. = 1.8 a solution of formic acid and sodium formate, K a ×10–4 b. = 1.8 a solution of acetic acid and sodium acetate, K a ×10–5 c. = 3.5 a solution of hypochlorous acid and sodium hypochlorite, K a …
REVIEW QUESTIONS Chapter 8 - Los Angeles Mission College
1.5 mol 1 L 11. How many liters of a 5.0% (m/v) glucose solution would contain 75 g of glucose? 3 100 mL 1 L 75 g glucose x x = 1.5 L 5.0 g glucose 10 mL 12. A patient receives an IV containing …
pH and pOH Calculations - Just Only
3) Determine the pH of a 4.30 x 10-4 M NaOH solution. 4) If a solution is created by adding water to 2.30 x 10-4 moles of NaOH and 4.50 x 10-6 moles of HBr until the final volume is 1.00 L, what is …
Calculating pH and pOH worksheet - Everett Community College
concentration is of OH-) 4) A solution is created by measuring 3.60 -x 10-3 moles of NaOH and 5.95 x 104 moles of HCl into a container and then water is added until the final volume is 1.00 L. …
Aqueous Equilibria: Part II- Solubility Product PSI AP ... - NJCTL
Mar 31, 2012 · A) 5.0 x106 B) 1.2 x10-12 C) 1.6 x10-14 D) 5.0 x10-12 E) 5.0 x10-17 29) If 0.1 M aqueous solutions of the following pais of substances are combined, which pair will yield a …
7. SOLUTIONS OF ELECTROLYTES - Louisiana Tech University
K = 4.0 × 10–8 mol cm–3 = 4.0 × 10–5 mol dm–3 7.12. The concentration of the acid in water = 1500 ppm = 1500 g acid 106 g solution = 1.500 g acid 103 g solution = 1.500 g acid/60.05 g mol–1 1.00 …
Cambridge International AS & A Level - Exam-Mate
1148 –5.8 1176 –10.3 Assume the standard enthalpy change, o, and the standard entropy change, ∆H o∆, for this S reaction remain constant over this temperature range. (i) oUse the data in Table …
buffer is a solution that resists changes in pH upon the …
11. Circle the conjugate acid-base pair that you would choose to prepare a buffer solution that has a pH of4.50. a. HCIO and CIO' b. C6HsCOOH and C6HSCOO' c. HPO/' and P0. 43, (Ka 3.5 x 10'8) …
PSI AP Chemistry Aqueous Equilibria part II - NJCTL
What is the solubility (M) of Ni(OH) 2 in a solution buffered at pH = 11.5? The K sp of Ni(OH) 2 at 25oC is 6.0 x10-16. A) 6.0 x10-8 B) 1.1 x10-4 C) 1.9 x10-13 D) 6.0 x10-16 E) 5.9 x10-11. …
Chapter 16: Buffer Calculations – Answer Key Example 1 - FL
Example 2 - Buffer Method 2 What is the pH of a buffer made by adding 125mL of 0.14M HC 7H 5O 2 solution with 165mL of 0.16M NaC 7H 5O 2 solution?K a = 6.5 x 10-5 Need concentrations of …
1 pH and pOH - MIT OpenCourseWare
The pH of a solution is a measure of how acidic it is: a pH of 7 indicates the solution is neutral, while lower values are acidic and higher values are basic. The compliment to pH is pOH, a measure of …
LIQUID SOLUTION 7. 2 - ALLEN Career Institute
75% in an aqueous solution, the molality of the solution which shows a 2.5 K rise in the boiling point of the solution is _____ molal. (Rounded-off to the nearest integer) [K b –= 0.52K kg mol 1] 4 5. …
Unit 1 topic 10 ACIDS BASES pH & BUFFERS
of propanoic acid is 1.26 x 10-5 moldm-3. c) Give equations to show how the above solution fulfills its buffer function. d) Calculate the pH of the solution after 0.01 moles of NaOH are added to 500 …
Aqua Ammonia Info Manual - Airgas Specialty Products
0 4.862 1.374 x 10-5 5 4.830 1.479 x 10-5 10 4.804 1.570 x 10-5 15 4.782 1.652 x 10-5 20 4.767 1.710 x 10-5 25 4.751 1.774 x 10-5 30 4.740 1.820 x 10-5 35 4.733 1.849 x 10-5 ... solution is …
Buffer Solutions - Ms. Chui's science class
pH = 5.06 Calculations for basic buffer solutions are very similar. Example 3. Find the pH of a buffer solution that has 0.10 mol/L of NH3 and 0.050 mol/L NH4Cl. The Kbof NH3is 1.8 x 10-5. Logic: …
Chapter 7 Homework - UC Santa Barbara
2 29. The larger the K a the stronger the acid. a) HCl strong acid and H 2 O is a weak acid K w = K a (1.0×10-14) b) HNO 2 The K a of HNO 2 (4.0×10-4) > K w = K
Lab 9: Qualitative Analysis - Amazon Web Services, Inc.
2S to the above solution? (1pt) c. Assuming X has been removed, what are the identities of Q, W, Y and Z after the solution has been boiled? (2 pts) d. How do you confirm the identity of each …
Buffer solutions - uomus.edu.iq
Example: calculate the pH of a solution that is 0.2 M in NH 3 and 0.3 M in NH 4 Cl ( K b =1.75 x10-5) . Solution: -NH 4Cl → NH 4 + + Cl NH 4 + + H 2 O ⇌ NH 3 + H 3 O+ Ka = Kw Kb = 10 −14 1.75 x …
Aqueous and polar GPC/SEC columns - HPLC
PL aquagel-OH Guard 5 7.5 50 PL1149-1530 PL aquagel-OH Guard 8 7.5 50 PL1149-1840 PL aquagel-OH SEC columns PL aquagel-OH Analytical Column accessories Quantity (pk) Part No. …
OpenStax Chemistry 2e 14.1: Brønsted-Lowry Acids and …
OpenStax Chemistry 2e 14.1: Brønsted-Lowry Acids and Bases Page 5 of 43 Because K w increases with increasing temperature, the reaction in endothermic. When the temperature of the system is …
Selective Precipitation Calculations - University of California, …
Prof. Rob Corn - Chem M3LC Initial Solution has 1.00 mM Zn2+ and 1.00 mM Mg2+. Zinc and Magnesium Hydroxide Precipitation Zn(OH) 2(s) ⇌Zn2+ +2OH−Mg(OH) 2(s) ⇌Mg2+ +2OH−K …
Test2 ch17a Acid-Base Practice Problems - Minnesota State …
34. Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, Ka? a. 5.25 …
A 0.10 M solution of formic acid (HCHO2) has a pH of 2
A 0.10 M solution of formic acid (HCHO2) has a pH of 3.2999999999999998at 25°C (a) Calculate Ka for formic acid at this temperature. pH = - log [H+] = 3.2999999999999998
Exp 16 Buffer solution Sp07 - Cerritos College
pH OF AMMONIUM ACETATE SOLUTION: 1. Measure the pH of 1.0 M NH 4C 2H 3O 2 solution. Record your result and answer the questions on your report sheet. AMMONIUM ACETATE AS A …
11. The concentration of hydroxide ions, OH C is 0.150 mol/L. O
140 MHR Chemistry 12 Solutions Manual 978-0-07-106042-4 18. A solution has a hydronium ion, H 3O +(aq), concentration of 0.152 mol/L at 25 °C.What is the hydroxide ion, OH –(aq), …
Chapter 16 Acid-Base Equilibria and Solubility Equilibria
28. Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of 0.10 M HCN (Ka = 4.9 × 10-10) solution. A. 5.15 B. 8.71 C. 5.85 D. 9.91 E. 13.0 29. Methyl …
1.3 – Worksheet pH – pOH – [H ] – [ OH]
1.3 – Worksheet – KEY " pH – pOH – [H+] – [–OH] Pleasecompletethefollowingtable" pH" [H+]" [–OH]" pOH" 3.5" 3.2x10<4! 3.2x10<11! 10.5! 3.2! 5.8x10R4" 1 ...
Chapter 10 Solutions - WebAssign
c) ZnCrO4 no Rule 5 d) ZnCO3 no Rule 5 e) ZnS no Rule 5 27. Indicate all of the following compounds that could be used to make a 0.1-M solution of CrO42-ions: a) ZnCrO4 no Rule 5 b) …
childschemistry.weebly.com
c. Is the solution ac ic, c, or neutra . 0.0018M OH - Practice Makes Perfect! 1. A 1.0 x M NaOH solution has been prepared 2. A 6.5 x 10-1 M solution of HINO, has been prepared for an …
Chapter 16. Acid-Base Equilibria
Calculate the concentration of OH-in a 0.15M solution of NH 3. (1.6 x 10-3. M) Practice Problem 1 (16.15) What is the pH of a 0.65 M solution of pyridine, C. 5. H. 5. N? K. b ... to enough water to …
SOLUBILITY AND SOLUBILITY PRODUCT - uwo.ca
4 has K sp = 2.4 × 10 —5 and SrSO 4 has a K sp of 2.8 × 10 —7. (So SrSO 4 is less soluble.) A solution has a concentration of 0.10 M of both Ca 2+ and Sr ; then Na 2SO 4(s) is slowly added. …
Lab 8: Ksp of Ca(OH)2 - Labflow
2) Add 5 drops of phenolphthalein to each flask and swirl. The solution should be hot pink. 3) Obtain 50-100mL of HCl titration solution in one of the 250 mL beakers, record the HCl concentration …
Scanned Documents - Colby College
May 2, 2019 · OH- —x Knowledge Required: How to 'ATite an equilibrium expression. (2) How to combtne multiple chemical ... dissolve, and a heterogeneous solution has formed. You know this …
Practice Test: Acids & Bases - Prexams
unknown HCl solution? (A) 1.2 M (C) 0.30 M (B) 0.13 M (D) 0.090 M ____17. According to the Arrhenius theory, the acidic property of an aqueous solution is due to an excess of (A) H 2 (B) H+ …
SOLVING SOLUTION AND MIXTURE VERBAL PROBLEMS 1.
the concentration if the resulting solution has a 14% concentration? 11. Mixed Nuts has 10% pecans. Nestor Nuts has 18% pecans. How many ounces of each should be mixed to get 20 ounces of a …
Turlock High AP CHEMISTRY - Class Data
volumetric pipet to deliver the propanoic acid solution to a clean, dry flask. After adding an appropriate indicator to the flask, the student titrates the solution with the 0, 173 M NaOH, …
CHAPTER 7 ACIDS AND BASES - Prexams
5 H 5 NH +(aq) + OH (aq) K = K b = [C H N] [C H NH ][OH ] 5 5 5 5 17. An acid is a proton (H+) donor, and a base is a proton acceptor. A conjugate acid-base pair differs by only a proton (H+) …
CHEMISTRY 1AA3-TUTORIAL 3 SOLUTIONS WEEK OF …
2O HNO2 + OH-Therefore, this solution is basic. c) (C5H5NH)ClO4 → C5H5NH + + ClO 4-C5H5NH + is the conjugate acid of C 5H5N, a weak base, so it is a weak acid: C5H5NH + + H 2O C5H5N + …
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