Calculate the pH and concentration of species present in a polyprotic acid solution.

Question

Question

For a 3.44×10^-3 M solution ofH₂CO₃, calculate both the pH and the CO₃^2- ion concentration.

H₂CO₃ + H₂O → H₃O⁺ +HCO₃^-					K_a1 = 4.2×10^-7
HCO₃^- + H₂O → H₃O⁺ +CO₃^2-					K_a2 = 4.8×10^-11

pH =
[CO₃^2-] =

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

Tutored Practice Problem 17.3.5 COUNTS TOWAIDA CHEE Calculate the pH and concentration of species present in...

Tutored Practice Problem 17.3.5 COUNTS TOWAIDA CHEE Calculate the pH and concentration of species present in a polyprotic acid solution. Close Problem For a 5.96X10 M solution of H2CO3, calculate both the pH and the Co, ion concentration. H2CO3 + H20= HCO3 + H20= H20* + HCO3 K1 = 4.2*10-7 H30* +CO;2- K2 -4.810-11 pH (CO3? Check & Submit Answer Show Approach Polyprotic Acid Titration Plots The pH plot for the titration of the diprotic acid maleic acid, HOC(CH), CO,H,...
Calculate the pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2–...

Calculate the pH and the concentrations of all species present (H2CO3, HCO3 – , CO3 2– , H3O + , and OH– ) in a 0.0037 M M carbonic acid solution. Ka1 = 4.3 × 10–7 ; Ka2 = 5.6 × 10–11
Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a...

Worksheet 19 Titration of Polyprotic Acids Name: 1. Calculate the sulfite ion [SO3'] concentration in a 0.123 M solution of the weak acid, sulfurous acid (H2SO3). The stepwise dissociation constants of carbonic acid are: Ka1 1.41 x 102 Ka2-6.31 x 108 3. Consider the following dissociation of the triprotic acid, phosphoric acid (HsPOs): Step 1 H3POa + H2O <=> H30+ + H2PO4, Step 2 HP0i + H2O <=> H30+ + HP042- Step 3 HPO42-+ H2O <-> H3O+ + PO43- Kal=7.1...

a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid...

a) Find the concentration of H+, HCO3- and CO32-, in a 0.01M solution of carbonic acid if the pH of this is 4.18. Ka1 (H2CO3) =4.45 x 10–7 and Ka2 =4.69 x 10–11 (b) Calculate the pH at the equivalence point of the titration between 0.1M CH3COOH (25 ml) with 0.05 M NaOH. Ka (CH3COOH) = 1.8 x 10–5.
The pH of a bicarbonate-carbonic acid buffer is 6.62. Calculate the ratio of the concentration of...

The pH of a bicarbonate-carbonic acid buffer is 6.62. Calculate the ratio of the concentration of carbonic acid ( H2CO3 ) to that of the bicarbonate ion ( HCO3− ). ( Ka1 of carbonic acid is 4.2 × 10−7. ) [ H2CO3 ]/ [ HCO3− ] =
The pH of a bicarbonate-carbonic acid buffer is 5.96. Calculate the ratio of the concentration of...

The pH of a bicarbonate-carbonic acid buffer is 5.96. Calculate the ratio of the concentration of carbonic acid (H2CO3) to that of the bicarbonate ion (HCO3−).(Ka1 of carbonic acid is 4.2 × 10−7.) [ H2CO3 ] [ HCO3− ] =

1) Consider a 0.040 M solution of carbonic acid. Calculate the pH of this solution as well as the equilibrium concentra...

1) Consider a 0.040 M solution of carbonic acid. Calculate the pH of this solution as well as the equilibrium concentrations of: [H2CO3], [HCO3-], [H3O+], and [CO32-). H2CO3 + H20 5 HCO3 + H30+ K1 = 4.45 x 10-7 HCO3 + H20 5 CO32- + H30+ K2 = 4.69 x 10-11
What is the pH of a 0.10 M solution of carbonic acid? Carbonic acid, H2CO3 has...

What is the pH of a 0.10 M solution of carbonic acid? Carbonic acid, H2CO3 has two acidic protons: H2CO3 + H2O7 HCO3 + H30+ Ka1 = 4.3x10-7 HCO3 + H202 CO32- + H30+ Ka2 = 5.6x10-11 a) 1.00 b) 0.70 c) 6.37 d) 3.68 e) I still can't figure this out...
12. Calculate the pH and the concentration of all species in solution of 0.33 M K2CO3....

12. Calculate the pH and the concentration of all species in solution of 0.33 M K2CO3. For carbonic acid Ka1 = 4.3 x 10-7 and Ka2 = 5.6 x 10-11

A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3]...

A 100.00 mL buffer solution at pH 7.80 is prepared such that the [H2CO3] + [HCO3] = 1.000 M. Determine how much strong acid 1.00M HCI or strong base 1.000 M NaOH must be added to change the pH to 7.40. The step-wise acid dissociation constants for carbonic acid are Ka1= 4.2*10^-7 ; Ka2= 4.8*10^-11.