## Question

###### The larger Ka (smaller pKa), the smaller Kb (larger pKt): Stronger the acid, weaker its conjugate base, and vice versaCalculate Kb for the base F- anion if Ka = 6.8 x 10 ^ for HFCalculate Ka for NHa* if given Kt = 1.8 x 10-5 for NHz:For a 0.20 M NaF solution, calculate Kb' [OH:]; pOH, pH. Ka = 6.8 x 10 4For 0.15 M NHACI, find pH NH3 has a Kb = 1.8 X 10-5.For HCN, Ks = 4.9x 10-10_ Calculate [OH:], pH, [HCN] for a 0.010 Maqueous solution of sodium cyanide, NaCN: CHEM 1516 Loekmw

The larger Ka (smaller pKa), the smaller Kb (larger pKt): Stronger the acid, weaker its conjugate base, and vice versa Calculate Kb for the base F- anion if Ka = 6.8 x 10 ^ for HF Calculate Ka for NHa* if given Kt = 1.8 x 10-5 for NHz: For a 0.20 M NaF solution, calculate Kb' [OH:]; pOH, pH. Ka = 6.8 x 10 4 For 0.15 M NHACI, find pH NH3 has a Kb = 1.8 X 10-5. For HCN, Ks = 4.9x 10-10_ Calculate [OH:], pH, [HCN] for a 0.010 Maqueous solution of sodium cyanide, NaCN: CHEM 1516 Loekmw

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