Q3.This question is about the pH of several solutions.Give all values of pH to 2 decimal places.(a) (i)Write an expression for pH.(b)(ii)Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³hydrochloric acid are added to 990 cm³ of water.The acid dissociation constant, Ka, for the weak acid HX has the value4.83 x 10-5 mol dm-³ at 25 °C.A solution of HX has a pH of 2.48Calculate the concentration of HX in the solution.Page 4 of 14

PH of solution determines the nature of solution whether it is acid or basic solution. The acidic…

Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-3 hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution.

Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-3 hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the pH of a 0.0307 M aqueous solution of nitrous acid (HNO₂, K₂ = 4.5×10-4). pH =
The initial molar concentration of formic acid (HCOOH) is 1.7 M. What is the pH of the solution, if the ionization constant for acetic acid is Ka= 1.7×10–4? Enter your answer with correct units and significant figures.
Whats the ph?
(a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?
A solution is made by dissolving 28.1 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 × 10⁻¹¹, determine the pH of the solution.
1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.061 M. 2.) We place 0.149 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.11 . Calculate the ionization contant, Ka, of HA. 3.)We place 0.527 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.35 . Calculate the ionization constant, Ka, of HA.
A solution is made by dissolving 25.1 g of Ba(NO₂)₂ in 500.0 mL of water. Using Kb(NO₂⁻) = 2.2 × 10⁻¹¹, determine the pH of the solution.
Give correct handwritten answer
Ammonia, a weak base with a Kb value of 1.8 x 10^-5 (a) What is the pH of a 0.155 mol L^-1 ammonia solution? (b) What is the percent ionization of ammonia at this concentration?
1A) Calculate the concentration of C5H5N solution required to provide a pH of 9.29. The Kb of C5H5N is 1.7 × 10-9 at 25°C. 1B) Calculate the mass of C5H5N needed to prepare 2.20 L of the above solution. (Molar mass = 79.10 g/ mol) 2A) The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10, What is the pH of an aqueous solution of 0.80 M sodium cyanide (NaCN)? 2B) What would be pH of the above solution if NaCN was a strong base? 3A) Write the conjugate base of the following: a) C7H602. b) HCO3- c) ) HASO3²- 3B) Write the conjugate acid of the following: a) PH3 b) SiO32- c) BrO3" 3C) Using 3A-a (C7H6O2) and its conjugate-base as an example, prove that "KąKp = Kw" Search or type URL く=
Hydrochloric acid is one of the common acids used in the laboratory. It is a very strong acid and react with many substances including metals. (a) Why is hydrochloric acid classified as a strong acid? (b) Write a chemical equation to represent its action on zinc (c) What is observed when: litmus paper is dipped in hydrochloric acid? two drops of methyl orange is put in 20cm3 of 0.1M hydrochloric acid? iii. Hydrochloric acid react with calcium carbonate
you prepare a solution of 3.1 x 10-8M KOH and calculate the pH in the typical way for a strong base: calculate pOH (7.51), then pH = 6.49. When you place a pH meter in the solution you find that the pH is actually 7.11. What was wrong with your calculation? (Brief conceptual explanation is fine here – no calculations needed.)