The standardized barium hydroxide solution is then used to titrate 10.95 mL of a

Q: The standardized barium hydroxide solution is then used to titrate 10.95 mL of a

2 HCOOH + Ba(OH)2 ----> Ba(COOH)2 + H2O(L) from equation : 2 mol HCOOH = 1 mol Ba(OH) 2 M1V1/n1 = M2V2/n2 let us assume , M2 = molarity of Ba(OH)2 = 1 M M1*10.95/2 = 33.82*1/1 M1 = molarity (in mol/L) of the formic acid solution = 6.18 M Note : if molarity of Ba(OH)2 is different the molarity (in mol/L) of the formic acid solution changes.

ID: 922976 • Letter: T

Question

The standardized barium hydroxide solution is then used to titrate 10.95 mL of a solution of formic acid (HCOOH). An endpoint is reached when 33.82 mL of barium hydroxide has been added. Determine the molarity (in mol/L) of the formic acid solution. Report your answer to four significant figures. The standardized barium hydroxide solution is then used to titrate 10.95 mL of a solution of formic acid (HCOOH). An endpoint is reached when 33.82 mL of barium hydroxide has been added. Determine the molarity (in mol/L) of the formic acid solution. Report your answer to four significant figures.

Explanation / Answer

2 HCOOH + Ba(OH)2 ----> Ba(COOH)2 + H2O(L)

from equation : 2 mol HCOOH = 1 mol Ba(OH) 2

M1V1/n1 = M2V2/n2

let us assume , M2 = molarity of Ba(OH)2 = 1 M

M1*10.95/2 = 33.82*1/1

M1 = molarity (in mol/L) of the formic acid solution = 6.18 M

Note : if molarity of Ba(OH)2 is different the molarity (in mol/L) of the formic acid solution changes.

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The standardized barium hydroxide solution is then used to titrate 10.95 mL of a

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