Suppose 1.36 mol of HCl is dissolved in enough water to give 807.0 mL of solutio

Question

Suppose 1.36 mol of HCl is dissolved in enough water to give 807.0 mL of solution. What is the H3O+ concentration? [Hint: When 1 mole of HCl dissociates, we get 1 mole of H3O+ ion because the acid is strong and monoprotic. Your answer should be in moles of H3O+ per liter of solution.] What is the OH- concentration? [Hint: Use the Kw relationship.] Suppose 1.36 mol of HCl is dissolved in enough water to give 807.0 mL of solution. What is the H3O+ concentration? [Hint: When 1 mole of HCl dissociates, we get 1 mole of H3O+ ion because the acid is strong and monoprotic. Your answer should be in moles of H3O+ per liter of solution.] What is the OH- concentration? [Hint: Use the Kw relationship.] What is the H3O+ concentration? [Hint: When 1 mole of HCl dissociates, we get 1 mole of H3O+ ion because the acid is strong and monoprotic. Your answer should be in moles of H3O+ per liter of solution.] What is the OH- concentration? [Hint: Use the Kw relationship.]

Explanation / Answer

Molarity(M) = (n)*(1000/V)

n = 1.36 mol

v = vol of solution = 807 ml

Molarity = 1.36*(1000/807) = 1.685 M

concentration of H3O+ = 1.685 M

concentration of H3O+ = 1.685 mol/L

kw = [H3O+][OH-]

10^-14 = 1.685*X

X = [OH-] = 5.93*10^-15 M

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