#1) Write the equation that shows the acid-base reaction of ammonia, NH3, and hy

Question

#1) Write the equation that shows the acid-base reaction of ammonia, NH3, and hydrobromic acid, HBr.

#2) Consider the extent of ionization for three acids, which has the largest Ka and which the smallest?

0.10 M HC3H5O3(aq) 3.7% ionization

0.10 M HClO2(aq) 28% ionization

0.10 M Al^3+ (aq) 1.2% ionization

#3) A solution containing 0.50 moles of the weak acid HBrO2 was found to have a pH of 2.8. Addition of 0.50 moles of NaBrO2 would have what effect on this solution?

A. The solution pH would increase.

B. The solution pH would decrease then return to approximately 2.8.

C. The solution pH would not change appreciably.

D. The solution pH would decrease.

#4) A solution is composed of equal concentrations of aqueous ammonia (pKb= 4.74) and ammonium chloride (pKa= 9.26). What would be the pH of the resulting solution?

A. 9.26

B. 4.74

C. The pH of the solution cannot be determined from the information given.

D. 7.00

Explanation / Answer

Write the equation that shows the acid-base reaction of ammonia, NH3, and hydrobromic acid, HBr.

NH3 (aq)+ HBr(aq) --> NH4+ (aq)+ Br- (aq)

#2) Consider the extent of ionization for three acids, which has the largest Ka and which the smallest?

0.10 M HC3H5O3(aq) 3.7% ionization largest Ka

0.10 M HClO2(aq) 28% ionization smallest ka

0.10 M Al^3+ (aq) 1.2% ionization

#3) A solution containing 0.50 moles of the weak acid HBrO2 was found to have a pH of 2.8. Addition of 0.50 moles of NaBrO2 would have what effect on this solution?

C. The solution pH would not change appreciably.

#4) A solution is composed of equal concentrations of aqueous ammonia (pKb= 4.74) and ammonium chloride (pKa= 9.26). What would be the pH of the resulting solution?

B. 4.74

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