How much of a 21.0 M hydrochloric acid solution would you dilute to prepare 50.00 mL of 9.00 M HCl?

How much of a 21.0 M hydrochloric acid solution would you dilute to prepare 50.00 mL...
Question 1: In the laboratory you dilute 3.33 mL of a concentrated 6.00 M hydrochloric acid solution to a total volume of 75.0 mL. What is the concentration of the dilute solution? M Question 2: You wish to make a 0.153 M hydroiodic acid solution from a stock solution of 3.00 M hydroiodic acid. How much concentrated acid must you add to obtain a total volume of 100 mL of the dilute solution? mL Thank-you!
In the laboratory, you dilute 3.61 mL of a concentrated 12.0 M hydrochloric acid solution to a total volume of 175 mL. What is the concentration of the dilute solution?
To standardize a solution of hydrochloric acid, you put 50.00 mL of it in a flask with a few drops of an indicator. You place 0.1524 M barium hydroxide in the buret. The buret reads 0.55 mL at the start and 33.87 mL when the equivalence point was reached. What is the molarity of the hydrochloric acid solution?
You wish to make a 0.445 M hydrochloric acid solution from a stock solution of 12.0 M hydrochloric acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution?
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
You want to dilute a 6.00 M HCl solution to 3.01 M. You need 500. mL of the diluted solution. How much stock solution (6.00 M HCl) must you use? Give your answer in mL.
The initial concentration of hydrochloric acid, HCl, is 12 M. I want to dilute this solution to get 500. 5. 0 mL of a 1.5 M solution. How many mL of the concentrated HCI must I use? 6. How many moles of sodium carbonate are contained in 200.00 mL of an 0.835 M solution of Na2CO3? 7. For the following reaction: 3 Cu(o+ 4 HNOs (a)3 Cu(NO,)2 (0)+2 NO20)+2 H20 What volume of 0.285 M HNOs is required for complete...
You wish to make a 0.253 M hydroiodic acid solution from a stock solution of 12.0 M hydroiodic acid. How much concentrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? in mL In the laboratory you dilute 2.31 mL of a concentrated 6.00 M hydrobromic acid solution to a total volume of 100 mL. What is the concentration of the dilute solution? You wish to make a 0.388 M hydrochloric acid solution...
Commercial hydrochloric acid is available as a 10.17 molar solution. How would you use this to prepare 200 mL of a 1.00 molar solution? Select one: O a. 19.7 mL of HCl +water to make the total solution volume of 200 ml O b. 1.97 mL of HCI + water to make the total solution volume of 200 ml O C. 1.97 mL of HCl + 200 mL of water O d. 19.7 mL of HCI + 200 mL of...
How could you make 2.5 L of 0.10 M hydrochloric acid?
Question 10 (1 point) How could you make 2.5 L of 0.10 M hydrochloric acid? Hint: This is a dilution. How many moles of HCI in 2.5L of 0.1M? Use the fact that M = ? that M - n moles so # of moles n = M, V =.. O dilute 59.4 mL of 3.0 M HCl to 2.5 L with water O dilute 0.25 L of pure...