A solution of sodium chlorite is prepared using 0.38 mol L1 NaOH as the solvent. The pK, of chlorous acid is 2. The concentration of sodium chlorite after mixing, before any reaction takes place is 0.24 mol L1. Calculate the equilibrium concentrations of all acid species: [ HCIO2 ], [ CIO2 ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correc assumptions first, the quadratic formula will give you the wrong answer. [ HCIO2 ) mol L'1, [ CIO2 ) - mol L1, pH = pOH

A solution of sodium chlorite is prepared using 0.38 mol L1 NaOH as the solvent. The pK, of chlorous acid is 2. The concentration of sodium chlorite after mixing, before any reaction takes place is 0.24 mol L1. Calculate the equilibrium concentrations of all acid species: [ HCIO2 ], [ CIO2 ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correc assumptions first, the quadratic formula will give you the wrong answer. [ HCIO2 ) mol L'1, [ CIO2 ) - mol L1, pH = pOH

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

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NO, (aq) + H20 ()=HNO, (aq) + OH¯ (aq) K =
Determine the pH at the equivalence (stoichiometric) point in the titration of 48.38 mL of 0.171 M HCN (aq) with 0.135 M NaOH(aq). The Ka of HCN is 4.9 * 10^-10.
You are on a new planet and discover a substance, Z2O that undergoes autoionization just like water on Earth. Z2O + Z2O ⇌ Z3O+ + OZ– Through a series of experiments, you determine the equilibrium constant (Kx) for this autoionization reaction at various temperatures. The value of Keq at 26.8ºC is 6.9 x 10-14. What is the pZ of the pure substance at this temperature? (pZ = -log(Z3O+) Report your answer to the hundreths place
Sulfuric acid (H2SO4) is a diprotic acid where the first deprotonation is a strong acid process, and the second deprotonation is a weak acid process with Ka = 1.0 x 10-2. What is the pH of a 0.00075 M solution of sulfuric acid?
We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?
Consider the titration of 25.00 cm3 of 0.10 M CH3COOH(aq) with 0.20 M NaOH(aq) at 25 °C. Calculate the pH of the solution after the addition of 5.00 cm3 of the titrant to the analyte in the titration.
5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.
2. Dr. Dahm has prepared 250 mL of a acetate buffer which contains 0.1 mol of acetic acid (CH₂COOH) and 0.15 moles of acetate (CH₂COO). Determine the initial pH. If he then adds 0.025 moles of H* calculate the new pH. Ka = 1.8 × 10³ CH₂COOH(aq) + H₂O CH₂COO (aq) + HO (aq) 3. Dr. Dahm makes a second acetate buffer exactly the same way as in #2, but he then adds 15 mL of 0.50 M NaOH calculate the new pH.
What would be the equation for equilibrium constant for the following reaction? 4 Pb(OH)4 (aq) + 2H₂SO4 (aq) = Pb(SO4)2 (aq) + 4H₂O (1) OK= PM(OH), H₂SO0,] [P(SO), H₂O] 74 0 PHOH), H₂SO [Pb(SQ),] PL(SO), H₂O Pb(OH) [H₂SO4)² Pb(SO₂),,O [PHOH), H, SO₂] OK = OK (= O None of the above
(vi) HCN is a weak acid with a Ka of 4.9 x 10-10. Write an equilibrium expression for this process and calculate the pH for a 0.4 mol L-1 solution of HCN.
To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should be measured (HCO3-+CO2), this was determined by acidifying the sample and measuring the volume of CO2 released. The concentration of H2CO3 was 28.5 mmol/L, the pH of the blood at 37 ℃ is 7.48 with a pka of 6.10, what is the concentration of HCO3- in mmol/L in the blood? a) 27.36b) 22.77c) 28.50d) 29.60
A brand of window-cleaning fluid is composed of ammonia solution, water, a colouring agent, and a very small quantity of soap. It has 0.15 mol/L concentration of NH3(aq). What is the pH of this fluid?