You are given the dissociation reactions of sulfuric acid: H₂SO4(aq) + H₂O(1)→ H3O+ (aq) + HSO4 (aq) Strong HSO₂ (aq) + H₂O(1) H₂O¹(aq) + SO4²- (aq) K₁₂ = 0.012 In order to calculate the pH of 0.1M sulfuric acid, you will: A) Calculate [H3O+] from the first reaction (100% ionization); second reaction is insignificant B) Calculate [H3O+] from the second reaction C) Take into account [H3O+] concentrations from both reactions

You are given the dissociation reactions of sulfuric acid: H₂SO4(aq) + H₂O(1)→ H3O+ (aq) + HSO4 (aq) Strong HSO₂ (aq) + H₂O(1) H₂O¹(aq) + SO4²- (aq) K₁₂ = 0.012 In order to calculate the pH of 0.1M sulfuric acid, you will: A) Calculate [H3O+] from the first reaction (100% ionization); second reaction is insignificant B) Calculate [H3O+] from the second reaction C) Take into account [H3O+] concentrations from both reactions

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the pH of 1mol dm-3 potassium hydroxide (KOH(aq)) KOH( aq) K+ (aq) + OH- (aq)
For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. reaction HCl(aq) + H₂O(1) → CI¯ (aq) + H₂O* (aq) NH (aq) + H,O →+ NH,(aq) + HạO (aq) Cl(aq) + H₂O(1) → HCl(aq) + OH (aq) NH3(aq) + H₂O(1)→ NH(aq) + OH(aq) highlighted reactant Bronsted-Lowry Bronsted-Lowry neither acid base O O O
What is the general equation given when examining a titration? O A (aq) + H20 (1) = HA + OH (aq) (aq) H*e (aq) + ОН (aq) + OH' = H2O (1) О НА (aq) + H20 () =A (aq) + H3O*(aq) O HA (ag) + NaOH (ag) = NaA (aq) + H2O (1)
For the acid-base equilibrium, idicate the acid-base conjugate pairs. NH4(aq) + OH(aq) ➡ NH3(aq) + H2O(l) Hence Justify your answer
Boric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solution of boric acid? What is the degree of ionisation of boric acid in this solution? The hydrogen ion arises principally from the reaction: B(OH),(aq) + H,0(1) = B(OH)4 (aq) + H* (aq) The equilibrium constant for this reaction is 5.9 x 10-10
Give the explanation formula which using for the calculation.
In the given equation: HCOOH (aq) + H2O (l) ↔ H3O+ (aq) + HCOO– (aq), the initial concentration of formic acid is 0.58 M (Ka HCOOH = 1.78×10−4). What is the pH of formic acid?
Propanoic acid, CH₂CH₂COOH, is a weak monoprotic acid that is used to inhibit mould formation in bread. A student prepared a 0.10 mol/L solution of propanoic acid and found that the pH was 2.96. What is the acid dissociation constant for propanoic acid? [Hint: Setup an I.C.E. table] CH3CH₂COOH (aq) Ka for propanoic acid is: ←CH3CH₂COO (aq) + H (aq)
If 100.0 mL of 0.150 M Ca(OH)2 is reacted with 450.0 mL of 0.100 M HCL, what will be the pH of the resulting solution? Са(ОН)2 (аq) + HCI (aq) СаClz (aq) + Н2О (1)
Which of the following reactions is an acid-base reaction? A) AGNO:(aq) + KF(aq) → AgF(s) + KNO:(aq) B) NH:(aq) + HF(aq) → NH:"(aq) + -F(aq) C) NO: (aq) + AI(s) → NH3(g) + AIO: (aq) D) CH:(g) + 202(g) - 2H:O(g) + CO:(g)
The ionization constant of lactic acid, CH3CH(OH)CO2H, an acid found in the blood after strenuous exercise, is 1.36 × 10−4. If 20.0 g of lactic acid is used to make a solution with a volume of 1.00 L, what is the concentration of hydronium ion in the solution?
What is the pH of 0.1510 M selenious acid solution, H2SeO3? H2SeO3(aq) + H2O(l) → HSeO3−(aq) + H3O+(aq) Ka1 = 3.5000e-2 HSeO3−(aq) + H2O(l) → SeO32−(aq) + H3O+(aq) Ka2 = 5.0000e-8