Calculate the concentration and the pH in a .10 M solution of sodium acetate, Na(CH3CO2). Equilibrium...

Calculate the concentration and the pH in a .10 M solution of sodium acetate, Na(CH3CO2). Equilibrium constant of acetic is 1.8*10^-5.

Expert Solution

The dissociation of 0.10 sodium acetate CH3COONa yields 0.10 M acetate ion and 0.10 M Na⁺ ion.

CH₃COO^- (aq) + H₂O (l) <------------> CH₃COOH (aq) + OH^- (aq)

I(M) 0.10 - 0 0

C -x +x +x

Eq (0.10-x) x x

K_b = K_w/K_a = 5.55*10^-10 = (x)(x) / (0.10-x)

By solving - x = [OH^-] = 7.453*10^-6 M

Thus - pOH = -log [OH^-] = -log (7.453*10^-6 ) = 5.12

Hence - pH = 14 - 5.12 = 8.88

queen_honey_blossom answered 3 months ago

calculate the ph of .010 M sodium acetate

Calculate the pH and the equilibrium concentration of Se2- in a 8.75×10-2 M hydroselenic acid solution,...

Calculate the pH and the equilibrium concentration of Se2- in a 8.75×10-2 M hydroselenic acid solution, H2Se (aq). For H2Se, Ka1 = 1.3×10-4 and Ka2 = 1.0×10-11 pH = [Se2-] = M Calculate the pH and the equilibrium concentrations of HS- and S2- in a 0.0425 M hydrosulfuric acid solution, H2S (aq). For H2S, Ka1 = 1.0×10-7 and Ka2 = 1.0×10-19 pH = [HS-] = M [S2-] = M

Calculate the pH of a solution of 0.25 M Acetic acid and 0.34M Sodium acetate before...

Calculate the pH of a solution of 0.25 M Acetic acid and 0.34M Sodium acetate before and after 0.036 M NaOH is added to the solution. Ka of HAc = 1.8 x 10 -5 Please Use the ICE method

Calculate the pH of 0.10 M sodium acetate solution ( Ka, acetic acid = 1.76 x...

Calculate the pH of 0.10 M sodium acetate solution ( Ka, acetic acid = 1.76 x 10-5 ).

1. Calculate the hydronium ion concentration and pH for a 0.042 M solution of sodium formate,...

1. Calculate the hydronium ion concentration and pH for a 0.042 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11. [H3O+]----------------M pH--------------------- 2. What are the equilibrium concentrations of NH3, NH4+, and OH- in a 0.42 M solution of ammonia? What is the pH of the solution? Kb = 1.8 * 10^-5 [OH-] ----------------------- M [NH4+] ----------------------M [NH3] ---------------------- M pH----------------------------

Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2....

Calculate the hydronium ion concentration and pH for a 0.050 M solution of sodium formate, NaHCO2. Kb for reaction of HCO2- ion with water is 5.6 × 10-11. [H3O+] =_____ M pH =______

Calculate the pH of a solution made by adding 54 g of sodium acetate, NaCH3COO, to...

Calculate the pH of a solution made by adding 54 g of sodium acetate, NaCH3COO, to 12 g of acetic acid, CH3COOH, and dissolving in water to make 400. mL of solution.

1) What is the pH of a 0.246 M aqueous solution of sodium acetate, NaCH3COO? This...

1) What is the pH of a 0.246 M aqueous solution of sodium acetate, NaCH3COO? This solution is acidic, basic or neutral? 2) The substance benzoic acid (C6H5COOH) is a weak acid (Ka = 6.3×10-5). What is the pH of a 0.110 M aqueous solution of sodium benzoate, NaC6H5COO? This solution is acidic, basic or neutral? 3) What is the pH of a 9.17×10-2 M aqueous solution of ammonium nitrate, NH4NO3? This solution is acidic, basic or neutral?

What is the pH and the equilibrium concentration of PO43- in a 0.511 M solution of...

What is the pH and the equilibrium concentration of PO43- in a 0.511 M solution of H3PO4(aq)? Ka1=7.5*10-3, Ka2=6.2*10-8, Ka3=4.8*10-13

3. a) Calculate the pH of a sodium acetate-acetic acid buffer solution (Ka= 1.78 x 10-5)...

3. a) Calculate the pH of a sodium acetate-acetic acid buffer solution (Ka= 1.78 x 10-5) in which the concentration of both components is 1.0 M. What would be the pH of the solution if 1.5 mL of 0.50 M NaOH was added to 35.0 mL of the buffer? How much does the pH change? b) If the same amount and concentration of NaOH was added to 35.0 mL of pure water (initial pH = 7), what would be the...

Question