A 500 mL solution was prepared by diluting 2.00 mL of 10.5 mol/L HCl_(aq).The pH

Question

A 500 mL solution was prepared by diluting 2.00 mL of 10.5 mol/L HCl_(aq).The pH of the new solution is: 5.678 2.567 2.938 1.377 0.32 g of Ba(OH)_2(s) is dissolved in 1.0 L of water. The pH of the solution is 12.251 10.261 11.57 13.512 For which type of titration will the pH at equivalence point be basic (pH > 7)? a strong acid and a weak base a weak acid and a weak base strong acid and a strong base a weak acid and a strong base Which of these is amphiprotic (amphoteric)? H_2O HCO_3 SO_4^2 a and b Identify the conjugate base for HA in the following equation. HA + H_2O rightarrow A + H_3O H_2O H_3O^+ A^- HA Solution A has a pH of 5 and solution B has a pH of 8. Which has the greater concentration of OH ions? solution B solution A Solutions A and B have the same OH- concentrations impossible to tell Distilled water has a pH of 7.00 (neutral pH). Distilled water has no ions no H_3O^+ ions no OH^-ions [H_3O^+] = [OH^-) Which of the following bases would have the highest pH value? 0.1 mol/L NaOH 0.1 mol/L Ba(OH)_2 55.5 mol/L H_2O. 0.01 mol/L LiOH A 1.50 mold acid (HA) has a percent ionization of 3.3 %. What is the pH of the solution? 1.5 0.176 1.305 3.3 If K_a = 5.8 times 10^-10, then what is the value of K_b? 8.2 times 10 4 6.3 times 10^5 9.2 1.7 times 10^-5

Explanation / Answer

Ans(8)- (d) weak acid and strong base

this type of titration for ph >7

Ans(10)- the conjugate for the reaction will be A-

and Acid will be HA so the ans will be [C]

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