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6 Nov 2019
The questions are solving for:
You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1379 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 mL. You then take a 10.00 mL sample of the dilute acid solution and titrate it with the standard solution. You need 13.88 mL of the standard solution to reach the endpoint. What is the concentration of the original acid solution? Concentration = A 60.00 mL solution of 0.4500 M AgN03. was added to a solution of AsO43-. Ag3AsO4 precipitated and was filtered off. Fe3+ was added and the solution was titrated with 0.2400 M KSCN. After 36.90 mL of KSCN solution had been added, the solution turned red. What mass of ASO43- was in the original solution? Show transcribed image text
The questions are solving for:
You need to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. You have a 0.1379 M standard solution. You take a 25.00 mL sample of the original acid solution and dilute it to 250.0 mL. You then take a 10.00 mL sample of the dilute acid solution and titrate it with the standard solution. You need 13.88 mL of the standard solution to reach the endpoint. What is the concentration of the original acid solution? Concentration = A 60.00 mL solution of 0.4500 M AgN03. was added to a solution of AsO43-. Ag3AsO4 precipitated and was filtered off. Fe3+ was added and the solution was titrated with 0.2400 M KSCN. After 36.90 mL of KSCN solution had been added, the solution turned red. What mass of ASO43- was in the original solution?
Show transcribed image text Elin HesselLv2
15 Apr 2019