Use the sample data below to next 4 questions 10. The titration curve below repr

Question

Use the sample data below to next 4 questions 10. The titration curve below represents the titration of a weak acid with a strong base. BASE with Solid Acid Trial #1 | Acid | Base RATIO (NaOH) vol base / ass acid Final Value Initial 3.28 0.00 ml Value 2.56 2.50 mL Mass or Volume Used Trial #2 | Acid | Base | RATIO (NaOH) vol base mass acid kume ofbase adced( 1.85 45.50 ml What is the Ka of the weak acid? a) 1.6 x 10 b) 2.0 x 10 Final Value grams Initial 2.56 22.50 mL. Value Mass or Volume Used c) 1.0x 107 d) 1.0x 109 11. The salt produced by the reaction of an equal number of moles of KOH and HNO; will react with water to give a solution which is a) acidic. b) basic. c) neutral. 13. What is the percentage difference between d) non-ionic. e) impossible to the two calculated ratios for trials I and 2? a) 0.45 % b) 1,2 % c)24% d)3.5% determine. 14. Based on the answer to question #21, should this student run a third trial for Part 1? a) Yes c) More information is needed 12. If you mix 100. mL of 0.11 M HCI with 50.0 mL of 0.22 M NHs, what is the pH of the resulting solution? The K, of NH4 -5.6x10-10 a) 4.63 b) 5.19 c) 6.02 d) 8.37 e) 9.37 15. If the solid acid used above was potassium hydrogen tartrate (KHC HaOs M.W. 188.15), how many moles oroE in trial #1 were needed to completely neutralize the acid? a) 0.0174 moles b) 0.00766 moles c) 0.00377 moles d) 0.00383 moles

Explanation / Answer

10)

a) 1.6*10 -4

for a weak acid vs strong base, pKa = 1/2(pH at end point)

pH at end point ~=8

therefore, pKa =-log(Ka) ~=4

Ka ~=1.6*10-4

11) c

A salt formed from a strong acid and a strong base is neutral.

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