Calculate the pH of 0.036 M nitrous acid (HNO2) solution: answer is 2.42. Please show all...

Calculate the pH of 0.036 M nitrous acid (HNO2) solution: answer is 2.42. Please show all steps.

Expert Solution

HNO2(aq) -------------> H^+ (aq) + NO2^- (aq)

I 0.036 0 0

C -x +x +x

E 0.036-x +x +x

Ka = [H^+][NO2^-]/[HNO2]

4.5*10^-4 = x*x/0.036-x

4.5*10^-4 *(0.036-x) = x^2

x = 0.0038

[H^+] = x = 0.0038M

PH = -log[H^+]

= -log0.0038

= 2.42 >>>>answer

queen_honey_blossom answered 1 year ago

Calculate the pH of a 0.0152 M aqueous solution of nitrous acid (HNO2, Ka = 4.6×10-4)...

Calculate the pH of a 0.0152 M aqueous solution of nitrous acid (HNO2, Ka = 4.6×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2]equilibrium = M [NO2- ]equilibrium = M

Be sure to answer all parts. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are...

Be sure to answer all parts. Exactly 100 mL of 0.15 M nitrous acid (HNO2) are titrated with a 0.15 M NaOH solution. (a) Calculate the pH for the initial solution. (b) Calculate the pH for the point at which 80.0 mL of the base has been added. (c) Calculate the pH for the equivalence point. (d) Calculate the pH for the point at which 105 mL of the base has been added.

Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous...

Calculate the percent ionization of nitrous acid in a solution that is 0.241 M in nitrous acid (HNO2) and 0.195 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 ⋅ 10-4.

Calculate the pH of the titration solution or 25.00 mL of 0.255 M nitrous acid nitrates...

Calculate the pH of the titration solution or 25.00 mL of 0.255 M nitrous acid nitrates with 0.214 M KOH at the following volumes of KOH: A. 0.00 mL B. 10.00 mL C. Mid-point of titration D. Equivalance point of titration E. 5.00 mL past equivalence point of titration

An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2)...

An analytical chemist is titrating 60.3 mL of a 0.5500 M solution of nitrous acid (HNO2) with a 0.6400 M solution of KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 22.2 mL of the KOH solution to it. Please round your answer to 2 decimal places

What is the pH of a 0.50 M solution of nitrous acid with a Ka of...

What is the pH of a 0.50 M solution of nitrous acid with a Ka of 4.0 x 10^-4?

Find the pH during the titration of 20.00 mL of 0.1000 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.1000 M nitrous acid, HNO2 (Ka = 7.1 10-4), with 0.1000 M NaOH solution after the following additions of titrant. Find at volumes of 0 mL, 10.00 mL, 15.00 mL, 20.00 mL, and 25.00 mL.

Find the pH during the titration of 20.00 mL of 0.2300 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.2300 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.2300 M NaOH solution after the following additions of titrant. a) 0mL b)10.00mL c) 15.00mL d) 19.00mL e)19.95 mL f) 20.00mL g) 20.05mL h) 25.00mL

Find the pH during the titration of 20.00 mL of 0.1820 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.1820 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.1820 M NaOH solution after the following additions of titrant. ( a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00 mL

Find the pH during the titration of 20.00 mL of 0.1590 M nitrous acid, HNO2 (Ka...

Find the pH during the titration of 20.00 mL of 0.1590 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.1590 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00 mL

Question