Homework Answers
to calculate no.of millimoles
use the last formula used for the calculation of molarity.
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5. you take 25.27 mL of a 0.572 M solution of K Cro, and dilute it...
PART 1: If you dilute 20.0 mL of 1.00 M hydrochloric acid to 750. mL, what...
PART 1: If you dilute 20.0 mL of 1.00 M hydrochloric acid to 750. mL, what is the molar concentration of the dilute acid? Molar concentration = ____________ M PART 2: If 7.00 mL of 0.0121 M CuSO4 is diluted to 10.0 mL with pure water, what is the molar concentration of copper(II) sulfate in the diluted solution? Molar concentration = ____________M
Suppose you have 100.00 mL of a solution of a dye and transfer 2.00 mL of...
Suppose you have 100.00 mL of a solution of a dye and transfer 2.00 mL of the solution to a 100.00 mL volumetric flask. After adding water to the 100.00 mL mark, you take 5.00 mL of that solution and again dilute to 100.00 mL. If you find the dye concentration in the final diluted sample is 0.000129 M, what was the dye concentration in the original solution? Concentration
If you dissolve 412 mg sucrose (formula weight: 342.29 g/mol) in 60 mL of water: a. What is the concentration of sucrose in mM in µM? b. If you take 5 mL of this solution and dilute it to 250 mL, what...
If you dissolve 412 mg sucrose (formula weight: 342.29 g/mol) in 60 mL of water: a. What is the concentration of sucrose in mM in µM? b. If you take 5 mL of this solution and dilute it to 250 mL, what is the concentration of the glucose in the resulting solution in µM? c. How many nano moles of sucrose are present in 10 mL of the diluted solution?
If you take a 15.0-mL portion of the stock solution and dilute it to a total...
If you take a 15.0-mL portion of the stock solution and dilute it to a total volume of 0.450 L , what will be the concentration of the final solution?
If you take a 10.0-mL portion of the stock solution and dilute it to a total...
If you take a 10.0-mL portion of the stock solution and dilute it to a total volume of 0.300 L , what will be the concentration of the final solution?
Question 3 If you dilute 25.00 mL of 0.90 M sodium phosphide solution to make 75.00...
Question 3 If you dilute 25.00 mL of 0.90 M sodium phosphide solution to make 75.00 mL of a new solution what is the new solutions concentration expressed as M of sodium ions? 2.7 M 0.90 M 0.45 M 0.30 M
25.00 g of potassium hydrogen phosphate (K HPO4) is dissolved in enough water to make 125.0...
25.00 g of potassium hydrogen phosphate (K HPO4) is dissolved in enough water to make 125.0 mL of a solution with a density of 1.22 g/mL. What is the concentration of the solution in % (m/m). % (m/v). molarity, mosM and mEq/L of the potassium ion? Note: K2HPO4 has a molar mass of 174.2g/mole. What would be the final molarity of the above solution if you were to dilute it by adding 175 mL of water?
If you dilute 17.0 mL of the stock solution to a final volume of 0.260 L...
If you dilute 17.0 mL of the stock solution to a final volume of 0.260 L , what will be the concentration of the diluted solution?
Dilution A chemist must dilute 67.1 ml of 2.92 M aqueous potassium iodide (KI) solution unti...
Dilution A chemist must dilute 67.1 ml of 2.92 M aqueous potassium iodide (KI) solution unti the concentration falls to 2.00 M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits mL 마10
an aliquot of 8 ml k2co3 solution that is 2.33 M is taken and diluted to...
an aliquot of 8 ml k2co3 solution that is 2.33 M is taken and diluted to a total volume of 250 ml. what is the concentration of potassium ions in solution?
Suppose you have 100.00 mL of a solution of a dye and transfer 2.00 mL of the solution to a 100.00 mL volumetric flask. After adding water to the 100.00 mL mark, you take 5.00 mL of that solution and again dilute to 100.00 mL. If you find the dye concentration in the final diluted sample is 0.000129 M, what was the dye concentration in the original solution? Concentration
Question 3 If you dilute 25.00 mL of 0.90 M sodium phosphide solution to make 75.00 mL of a new solution what is the new solutions concentration expressed as M of sodium ions? 2.7 M 0.90 M 0.45 M 0.30 M
Dilution A chemist must dilute 67.1 ml of 2.92 M aqueous potassium iodide (KI) solution unti the concentration falls to 2.00 M. He'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate this final volume, in milliliters. Round your answer to 3 significant digits mL 마10
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