Q22. Correct option is : (B) 13.26
Q23. Correct option is : (B) C9H7N (aq) + H2O (l) C9H7NH+ (aq) + OH- (aq)
Q24. Correct option is : (A) 1.8 x 10-6
Explanation
Q22. Given : hydroxide ion concentration, [OH-] = 0.18 M
pOH = -log[OH-]
pOH = -log(0.18 M)
pOH = 0.74
pH = 14 - pOH
pH = 14 - 0.74
pH = 13.26
2:12 al LTE Question 22 of 32 Submit A solution has a hydroxide-ion concentration of 0.18...
2:14 al LTE Question 25 of 32 Submit What is the Ka for a weak monoprotic acid (HA) if a 0.020 M solution of the acid has a pH of 3.23 at 25°C? A) 3.5 x 10-4 B) 5.9 x 10-2 C) 1.7 x 10-5 D) 1.2 x 10-6 2:14 al LTE Question 26 of 32 Submit What is the pH of a solution with an initial concentration of 0.42 M hypochlorous acid, HOCI (Ka = 3.0 x 10-9). A)...
2:06 LTE Question 29 of 32 Submit Which of the following would be the base equilibrium equation for CsCIO? A) CsCIO (aq) = Cs+ (aq) + CIO- (aq) B) CIO- (aq) + H20 (1) = CIOOH (aq) + H3O+ (aq) C) CIO- (aq) + H20 (1) = H2C1O2 (aq) D) CIO- (aq) + H20 (1) =HCIO (aq) + OH- (aq)
Find the hydronium ion concentration and pH for the following 1. 2. Calculate the hydronium ion concentration and the pH when 80.0 mL of 0.55 MNH, is mixed with 80.0 mL of 0.55 M HCl (K. = 5.6 x 10-10). Concentration M pH- Phenol (CH-OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(0) = CH.0 (aq) +H3O+ (aq) K= 1.3 x 10-10 If you dissolve 0.593 g of the acid in enough water to...
9) What is the H+ ion concentration in a 4.8 x 10–2 M KOH solution? A) 4.8 x 10–2 M B) 1.0x 10–7 M C) 2.1 x10–13 M D) 4.8 x 10–11 M 10) HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-? A) HA (aq) + H2O (l) H2A+ (aq) + OH-(aq) B) A- (aq) + H3O+ (aq) C) HA (aq) + OH- (aq) H2O (l) + H+ (aq) HA (aq) + H2O...
1:08 el LTE Question 13 of 32 Submit What is the hydronium-ion concentration of a 0.25 M HCl solution? A) 0.50 M B) 0.25 M C) 4.00 x 10-14 D) 1.00 x 10-7
The hydroxide ion concentration in an aqueous solution at 25°C is 4.4x10-2 M. The hydronium ion concentration is M. The pH of this solution is The pOH is The hydronium ion concentration in an aqueous solution at 25°C is 4.4x10 M. The hydroxide ion concentration is M. The pH of this solution is The pOH is Autoionization occurs when two solvent molecules collide and a proton is transferred between them. Write the autoionization reaction for water. Submit Answer Use pH,...
Question 27 What is the hydronium ion concentration in a 0.5 M ammonia solution? (1 point) 3.0E11 M 3.1E-15 M 3.3E-10 M 3.3E-12 M Question 28 Identify the conjugate acid in the following reaction, HNO3(aq) + H2O() - NO3- (aq) + H3O+ (aq). (1 point) H20 H30+ NO3- None of the above Question 29
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a pH of 2.0. Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 2. What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 3. Which is the stronger acid, NH4+ or HBrO? Hint: Compare...
30 5 points Determine the hydroxide ion concentration, [OH-], of a 0.125 M solution of the weak base NC3H5(Kfor NC3Hs is 1.7 x 109). NC3H5 (aq) + H20 (1) = HNC3H5+ (aq) + OH" (aq) O 6.8 x 10-8 M 1.5 x 10-5 M 1.2 x 10-4 M 2.1 x 10-10 M 2.1 x 10-4 M O O Previous Next
In the presence of excess OH-, the Al3+(aq) ion forms a hydroxide complex ion, Al(OH)4-. Calculate the concentration of free Al3+ ion when 1.32×10-2 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 13.00). For Al(OH)4-, Kf = 1.1×1033. [Al3+] = ?M