Starting with 300 mL of 0.75 M HCl, you want to dilute the solution to 0.25...
You have 505 mL of a 0.165 M HCl solution and you want to dilute it to exactly 0.100 M. How much water should you add? mL
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.
4. To what volume should you dilute 25 mL of a 10.0 M HCl solution to obtain a 0.250 M solution? Show your work Final Answer 5. Seawater has a concentration of 0.60 M NaCl. The acceptable amount of NaCi in drinking water is 9.0 g/L. How much pure water should be added to 2.50 L of seawater for it to be safe for human consumption? Show your work Final Answer
To what volume should you dilute 35 mL of a 13 M stock HCl solution to obtain a 0.580 M HCl solution?
To what volume should you dilute 35 mL of a 11 M stock HCl solution to obtain a 0.540 M HCl solution? Express your answer using two significant figures.
Using a 0.25 M phosphate buffer with a pH of 7.2, you add 0.75 mL of 0.55 M HCl to 57 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) Using a 0.25 M phosphate buffer with a pH of 7.2, you add 0.75 mL of 0.55 M NaOH to 57 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
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...
2. Calculate the pH of a solution prepared by diluting 0.25 mL of a 6.0 M HC red by diluting 0.25 mL of a 6.0 M HCl with water to a total 1.25 ml. Record this pH in Part I data sheet, Beaker #1 for Theoretical Final pH. 3. Calculate the pH of a solution prepared by dilutine 0.25 mL of a 6.0 M NaOH with water to a total volume of 20.25 mL. Record this pH in Part I...
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
A chemist must dilute 42.5 mL of 3.78 M aqueous iron(II) bromide (FeBr2) solution until 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