Which one of the following is a strong acid? NH_3 H_2SO_4 CH_2COOH HF HSO_4^- Wh

Question

Which one of the following is a strong acid? NH_3 H_2SO_4 CH_2COOH HF HSO_4^- What is the pH of a solution with [H^+] = 1.0 times 10^-5 M? 1.0 times 10^-3 3.0 5 -2.52 11.0 The [H_3O^+] in a 0.050 M solution of H_2SO_4 is: 1.0 times 10^-5 M 5.0 times 10^-2 M 5.0 times 10^-10 M 1.0 times 10^-1 M 2.0 times 10^-9 M The molar solubility of PbBr_2 is 2.17 times 10^-3 M at a certain temperature. Calculate K_sp for PbBr_2 6.2 times 10^-6 6.4 times 10^-7 1.4 times 10^-5 3.4 times 10^-6 4.1 times times 10^-8 What is the molar solubility, s, of AgCI in terms of K_ sp? s = [K_sp/4]^5 s = K_sp^1/5 s = [K_sp/27]^1/2 s = [K_sp/108]^1/2 s = K_sp^1/2 Which of the following salts has the lowest solubility? CuBr(K_sp = 6.3 times 10^-9) Cul(K_sp = 1.1 times 10^-12) AgBr(K_sp = 5.4 times 10^-13 CuCI(K_sp = 1.7 times 10^-7) AgI(K_sp = 8.5 times 10^-17) All of the following have delta G degree f notequalto 0 EXCEPT H_20(g) NO(g) HCI(g) CaO(s) Fe(s)

Explanation / Answer

13. B. H2So4

H2So4 is strong acid . it is completely ionisable in aqueous solution.

14. PH = -log[H+]

             = -log10-5

              = 5

C. 5

15. H2SO4 + H2O --------> H3O+ + HSO4-

     0.05M                           0.05M

   {H3O+] = 5*10-2 M

16. PbBr2 ---------> Pb+2 + 2Br-

                                s           2s

   Ksp = [Pb^+2][Br-]2

          = S*(2s)2

         = 4s3

        = 4*(2.17*10^-3)3

        = 4.1*10-8 >>>>Answe E

17. E

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