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Bookmarks Bookmarks People window He MasteringChemistry. Week 10 Assignment secure https: 75&offset-prev; CHEM 111-900 W17 Signed in as Sandra Pizarro Week 10Assignment Problem 11.74 previous l 24 of 26 l next Using the table below for Ka values, compare the pH of a Part A H2CO3 buffer that contains 0.13 M H2CO3 and 0.13 M What is the pH of a buffer solution containing 0.13 MEhoos and 0.13 M NaHcos? NaHCOa with another H2CO3 buffer that contains 0.21 Express your answer using two decimal places. M H2CO3 and 0.051 M NaHCO3 Ka and Kb Values for Selected Weak Acids and Bases Acids phoric acid HPO. 5 x 10 HNO2 4.5 x 10 Nitrous acid 3.5 x 10 Hydrofluoric acid HF My Answers Give Up 1.8 x 10 4 HCHO Formic acid HC H,02 1.8 x 10 Acetic acid Part B What is the pH of a buffer solution containing o.21 M Hacoa and 0.051 M NaHoos 4.3 x 10 H2CO3 Carbonic acid Hydrosulfuric acid H2S Express your answer using two decimal places. 62 x 10 Dihydrogen phosphate H,PO. 4.9 x 10 10 Hydrocyanic acid HCN 5.6 x 10 Hydrogen carbonate HCO, 2.2 x 10 Hydrogen phosphate HPO, My Answers Ghe Up 4.4 x 10 NH Methylamine 2.2 x 10 Carbonate NH Ammonia

Explanation / Answer

pH of acidic buffer we can calculate by using following equation.

pH = pKa + log [NaHCO3] /[H2CO3]

pKa = - log Ka = -log [4.3 x 10-7]

pKa = 6.37

pH = 6.37 + log [0.13] / [0.13]

pH = 6.37

part B)

pH = pKa + log [NaHCO3] / [H2CO3]

pH = 6.37 + log [0.051]/[0.21]

pH = 5.75

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