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.

(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.

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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.)