(b) An impure sample of (COOH)2.2H2O that had a mass of 1.00 g was dissolved in water and titrated with standard NaOH solution. The titration required 19.16 mL of 0.198 M NaOH solution. Calculate the percent (COOH)2.2H,O in the sample. Assume that the sample contains no acidic impurities. [molecular weight (COOH),.2H,O = 126 g/mol]
(b) An impure sample of (COOH)2.2H2O that had a mass of 1.00 g was dissolved in water and titrated with standard NaOH solution. The titration required 19.16 mL of 0.198 M NaOH solution. Calculate the percent (COOH)2.2H,O in the sample. Assume that the sample contains no acidic impurities. [molecular weight (COOH),.2H,O = 126 g/mol]
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Chapter14: Chemical Equilibrium
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![(b) An impure sample of (COOH)2.2H2O that had a mass of 1.00 g was dissolved in water and titrated with standard NaOH
solution. The titration required 19.16 mL of 0.198 M NaOH solution. Calculate the percent (COOH)2.2H,O in the sample.
Assume that the sample contains no acidic impurities. [molecular weight (COOH),.2H,O = 126 g/mol]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb09f6ecf-9e28-4d9a-8f0b-9234c2be33e5%2Fe2e10409-5829-4ccb-8d8e-82f64a5f6824%2Fsmloykd_processed.png&w=3840&q=75)
Transcribed Image Text:(b) An impure sample of (COOH)2.2H2O that had a mass of 1.00 g was dissolved in water and titrated with standard NaOH
solution. The titration required 19.16 mL of 0.198 M NaOH solution. Calculate the percent (COOH)2.2H,O in the sample.
Assume that the sample contains no acidic impurities. [molecular weight (COOH),.2H,O = 126 g/mol]
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