Which of the following compound cannot be a Bronsted-Lowry base? OH^- H_2O NH_3

Question

Which of the following compound cannot be a Bronsted-Lowry base? OH^- H_2O NH_3 NH^+_4 SH^- Suppose 0.50 L of a HNO_3 solution has a pH of 3.30. How many moles of HNO_3 must have been initially dissolved in the solution? 2.5 times 10^-4 moles 5.0 times 10^-4 moles 1.7 times 10^-4 moles 1.0 times 10^-3 moles 1.8 times 10^-2 moles A 0.100 M monoprotic weak acid solution has a pH of 3.00. What is the pK_a of this acid? 5.00 0.10 3.00 9.99 6.00 The solubility product for Al(OH)_3 is written as ________. K_sp = [Al^3+][OH^-]^3 K_sp = [Al^3+][OH^-]^3/[Al(OH)_3] K_sp = [Al^3+] 3[OH^-] K_sp = [Al^3+] + [OH^-]^3 K_sp = [Al^3+] 3[OH^-]/[Al(oH)_3]

Explanation / Answer

21) NH4+ cannot take H+ , so it is not Lewis base

22) H+ = 10-3.30 = 0.00050 M

Moles of HNO3 = 0.00050 M *0.50 L = 2.51*10-4 moles

23) H+ conc = 10-3 = 0.001 M

Ka =( 0.001)2 / (0.1) = 10-5

pKa = -log (10-5 ) = 5

24) Ksp =( Al3+)(OH-)3

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