What is [H3O+] and pH in a 0.10 M solution of HCN at 25

What is [H₃O+] and pH in a 0.10 M solution of HCN at 25

Expert Solution

We have , 0.10M HCN solution at 25^oc & Ka for HCN = 4.0 * 10^-10

HCN + H2O -----------> H3O⁺ + CN^-

Intial concentration 0.1 M 0 M 0 M

Change in concentration -x +X +X

Equilibrium concentration (0.1-x) X X

Ka = [H3O⁺][CN^-] / [HCN]

4.0 * 10^-10 = (X)(X) / (0.1-X)

4.0 * 10^-10 = (X)(X) / (0.1)

X² = (0.1) * (4.0 * 10^-10)

[H3O⁺] = X = 6.3 * 10^-6 M

[H3O⁺] = 6.3 * 10^-6 M

pH = -log[H3O⁺]

= -log (6.3 * 10-6)

pH = 5.2

queen_honey_blossom answered 2 years ago

What is [H3O+] and ph in a 0.10 M solution of HCN at 25 degrees celsius...

What is [H3O+] and ph in a 0.10 M solution of HCN at 25 degrees celsius (ka for HCN= 4.0x10-10) show steps

The pH of a 0.10 M HCN solution is 5.20. a. What is [H3O+ ] in...

The pH of a 0.10 M HCN solution is 5.20. a. What is [H3O+ ] in that solution? _______________ M b. What is [CN-]? What is [HCN]? (Where do the H+ and CN - ions come from?) [CN-] = _______________ M; [HCN] = _____________ M c. What is the value of Ka for HCN? What is the value of pKa? Ka = _______________ pKa = _______________

25 ml of 0.10 M CH3CO2H is titrated with 0.10 M NaOH. What is the pH...

25 ml of 0.10 M CH3CO2H is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH have been added? Ka for CH3CO2H = 1.8X10^-5

What is the concentration of hydronium ion, H3O + , in 0.10 M HClO at 25°C?...

What is the concentration of hydronium ion, H3O + , in 0.10 M HClO at 25°C? A. 3.0 × 10−8 M B. 3.0 × 10−7 M C. 5.5 × 10−5 M D. 1.7 × 10−4 M E. 0.10 M

Calculate the pH at 25 degree C of a solution formed by combining and 0.10 M...

Calculate the pH at 25 degree C of a solution formed by combining and 0.10 M HC2H3O2(aq) and 0.10 M NaC2H3O2(aq) Calculate the new pH formed after addition of 0.10 mol of HCl (aq) to 1.0 L of the solution formed in part (a)

a. What is the pH of a 0.040 M solution of HCN? Find the concentrations of...

a. What is the pH of a 0.040 M solution of HCN? Find the concentrations of all the major species in the solution? [HCN], [H3O+], [CN-]

What is the pH of a solution prepared by mixing 25 ml of 0.5 HCN with...

What is the pH of a solution prepared by mixing 25 ml of 0.5 HCN with 75 ml of 0.20 NaCN. Ka = 6.2*10^-10 for HCN. Hint: remember to dilutions first.

Calculate the [H3O^+] for a solution with pH= 11.50? A. What is the [H3O+] for a...

Calculate the [H3O^+] for a solution with pH= 11.50? A. What is the [H3O+] for a solution with pH = 11.50? B. What is the [OH^-] for the solution above? C. What is the [H3O+] for a solution with pH = 5.0? D. What is the [OH−] for the solution above? E. What is the [H3O+] for a solution with pH = 6.59? F. What is the [OH−] for the solution above? G. What is the [H3O+] for a solution...

Q1) A 0.10 M aqueous solution of sodium bromide has a pH __________ at 25°C. a)...

Q1) A 0.10 M aqueous solution of sodium bromide has a pH __________ at 25°C. a) less than 7.00 b) equal to 7.00 c) greater than 7.00 Q2) A 0.10 M aqueous solution of ammonium nitrate has a pH __________ at 25°C. a) less than 7.00 b)equal to 7.00 c)greater than 7.00 Q3 At 25ºC, the pH of a 0.10 M aqueous solution of an acid is 4.27. Find the value of Ka for this acid at 25ºC.{ give explanation...

20.0 ml of 0.10M HCN is titrated with 0.10 M KOH. determine the ph at the...

20.0 ml of 0.10M HCN is titrated with 0.10 M KOH. determine the ph at the equivalence point.

Question