Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <->...
Use the following chemical reaction a 6.8X1l0^-3 solution of carbonic acid: H2CO3 (aq) +H2O (l) <-> HCO3 (aq) + H3O . Ka1= 4.3x10^-7 . Ka2= 4.7x10^-11 a. if you add NaHCO3 to the solution, would the pH of the solution go up, down, or stay the same? b. Calculate the pH of the solution if you added 3.4 x10^-3 M NaHCO3.
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Use the following chemical reaction a 6.8X1l0^-3 solution of
carbonic acid: H2CO3 (aq) +H2O (l) <->...
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...
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic...
You create a 1 L solution of 0.1 M H2CO3. carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.5 x 10-7 and Ka2 = 4.7 x 10-11. a) What will the initial pH of the solution be? b) What volume of 0.1 M NaOH will you need to add to reach the second equivalence point( remember carbonic acid deprotonates to bicarbonate HCO3- and then can deprotonate further to CO32-? c) At the second equivalence point, what will the...
Match the substance to the correct label for the following reaction: H2CO3 (aq) + H2O (l) ⇔...
Match the substance to the correct label for the following reaction: H2CO3 (aq) + H2O (l) ⇔ H3O+(aq) + HCO3−(aq) Question 5 options: 1234 H2O 1234 H2CO3 1234 HCO3- 1234 H3O+ 1. Acid 2. Base 3. Conjugate acid 4. Conjugate base
Calculate the pH and concentration of species present in a polyprotic acid solution.
Calculate the pH and concentration of species present in a polyprotic acid solution.For a 3.44×10-3 M solution ofH2CO3, calculate both the pH and the CO32- ion concentration.H2CO3 + H2O → H3O+ +HCO3-Ka1 = 4.2×10-7HCO3- + H2O → H3O+ +CO32-Ka2 = 4.8×10-11pH =[CO32-] =
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated...
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...
Carbonic acid (H2CO3) is unstable in water and rapidly decomposes i to CO2(g) and H2O(l). Consequently,...
Carbonic acid (H2CO3) is unstable in water and rapidly decomposes i to CO2(g) and H2O(l). Consequently, the reaction between Coc-H+(aq) and HCO3-(aq) is better represented as
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of...
Find the pH of a 0.100 M carbonic acid (H2CO3) solution. Find the equilibrium concentration of CO3 -2. Ka1 = 4.30 x 10-7 Ka2 = 5.59 x 10-11
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×...
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 ×10-7 and Ka2 = 5.6 × 10-11.10)A) 10.44 B) 5.50 C) 4.31 D) 11.00 E) 3.56
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.
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beve...
a) The consecutive equilibria: CO2(g) <=>CO2(aq) + H2O(l) <=>H2CO3(aq) <=>H+(aq) + HCO3-(aq), explain why: A. carbonated beverages are less acidic than pure water. B. carbonated beverages contain measurably less water than the same volume of pure water. C. rainwater is slightly acidic b) A 1.0 M solution of a weak monoprotic acid with Ka = 1.0 10-6 would have a pH of: A. 1 B. 2 C. 3 D. 6 c) Ascorbic acid is a diprotic acid with Ka1 =...
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...
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