What is the pH of a solution which is 0.021 M in weak base and 0.039 M in the conjugate weak acid (K, = 7.1 x 10-)? pH =

What is the approximate K for the following acid/base reaction? H25 (aq) +F (aq) ++ HF (aq) +HS (aq) ACID BASE HCI C H2SO4 HNO3 H30 (aq) HSO H3PO4 HSO NO3 H2O so, H,PO, F HF CH3COOH H,CO3 H,S H,PO, NH, CH;COO HCO, HS HPO, NH, CO PO OH HCO HPO. 1,0 OH H, CH CH, OA unable to determine OB. K.<1 Base strength increasing Acid strength increasing

What is the pH of a solution with molar concentration of H*, [H*] = 1.0 x 10-9 M?

Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. CH:NH:CI(aq) + NaOH(aq) 4- 2+ | ]3+ 1 3 4 6 7 8 D4 15 Do ) (s) (1) (g) (aq) Na H C CI Reset • x H2O Delete 1L 2. +

The K, of a weak monoprotic acid is 1.65 x 10-5. What is the pH of a 0.0859 M solution of this acid? pH =

Determine the OH- and H+ concentration and calculate the pH, pOH of a solution that is 0.70 M NH3 solution. NH3 + H2O  <-->  NH4 + + OH-                     Kb = 1.8 x 10-5

20.

If the K, of a weak base is 2.4 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

3. Suppose 10-6 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This gives (H°] = (10-6 mol)/(1000 L) = 10-9 M. Finally, the pH is calculated: pH = -logro[H*]= -log-o{10 °) = 9.0, which corresponds to an alkaline solution! What is wrong? %3D %3D !! !3! 4. Calculate the pH of a 0.15 M solution of acetic acid, CH;COOH (K. = 1.8 x 109).

Calculate the pH of a 0.064-M Al (NO3)3 solution. The K, value for Al (H2O),* is 1.4 x 10-5. pH =