1
answer
0
watching
77
views
11 Nov 2019
Name Date Questions: In order to create a new solution of sodium hydroxide, a 6.00 M solution was used as the stock solution. If a total of 200L of -0.2 M NaOH is necessary to make, how many ml of the stock sodium hydroxide should be used to create this solution? 1. 2. Using the volume from the above question, calculate the real molarity of the NaOH that would be created using a 6.00 M solution and diluting it to 2.00 L. Assume we only have pipets for whole numbers capable of transferring whole number mL (Remember volumetric pipets have significant figures to the hundredths place.) 3. Why can't the solution made in Part B be tested to find the concentration experimentlly by titration with NaOH? 4. 25.00 mL. of a solution that contains an unknown amount of acetic acid is tested via titration with sodium hydroxide. Write the balanced chemical equation for this reaction. a. The sodium hydroxide had previously been standardized to be 0.1588 M and the titration required 22.54 mL. What is the mass of acetic acid present in the unknown? b.
Name Date Questions: In order to create a new solution of sodium hydroxide, a 6.00 M solution was used as the stock solution. If a total of 200L of -0.2 M NaOH is necessary to make, how many ml of the stock sodium hydroxide should be used to create this solution? 1. 2. Using the volume from the above question, calculate the real molarity of the NaOH that would be created using a 6.00 M solution and diluting it to 2.00 L. Assume we only have pipets for whole numbers capable of transferring whole number mL (Remember volumetric pipets have significant figures to the hundredths place.) 3. Why can't the solution made in Part B be tested to find the concentration experimentlly by titration with NaOH? 4. 25.00 mL. of a solution that contains an unknown amount of acetic acid is tested via titration with sodium hydroxide. Write the balanced chemical equation for this reaction. a. The sodium hydroxide had previously been standardized to be 0.1588 M and the titration required 22.54 mL. What is the mass of acetic acid present in the unknown? b.
Nelly StrackeLv2
11 Nov 2019