1- H2SO4 is a strong acid in its first ionization; but a weak acid in its second ionization with Ka = 0.012. Calculate the pH of a 0.056 M solution of H2SO4. O 0.012 0.0819 0.056

Which of the following 1.0 M solutions would have the highest pH? Weak Acid Ka Weak Base Kb HCN 4.9 x 10-10 HONH, 1.1 x 10-8 HNO2 4.5 x 104 NH3 1.8 x 10-5 HIO 2.3 x 10-11 CHINH, 4.3 x 10-10 HBrO 2.5 x 10-9 H¸NNH₂ 1.3 x 10-6 CHCOOH 6.3 x 105 CH N 1.7 x 10-9 A KCN B C CH NHCI Nalo + D NH Br

Identify the conjugation acid-base pairs in the following reactions. An acid donates a proton to become a conjugate base. A base accepts a proton to form a conjugate acid.

Conjugate acid of any base is defined as the species formed when the base accepts a proton. And the conjugate base of any acid is defined as the species formed when the base donates a proton. Hence in the conjugate acid-base pair, there will be a difference of 1 proton only. In the above reaction, the base NH3 is accepting a proton from the acid HF to form + NH4* ions. Hence NH3/NH4* is a conjugate acid-base pair. And the acid HF is donating a proton to form the conjugate base F. Hence HF/F is a conjugate acid-base pair. Hence the answer is NH3/NH4* & HF/F". ANSWER IN NO. 4