A student needs to dilute a 0.30 M Pb(NO,), solution to make 59.0 mL of 0.22...
A student needs to dilute a 0.34 M Pb(NO₃)₂ solution to make 81.0 mL of 0.18 M Pb(NO₃)₂. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.34 M Pb(NO₃)₂ solution that is needed.
I am wondering if this is right? Thanks A student needs to dilute a 0.28 M Pb(NO3), solution to make 111.0 mL of 0.11 M Pb(NO3)2. Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.28 M Pb(NO3)2 solution that is needed. 0.28 M 0.28 M x 0.11M) 0.11 M 4+ 2.7 x10-4 mL mL 111.0 mL Answer Bank 111.0 mL 111.0 ml 0.11 M 0.11...
Ch 11 HW nd Due Dates > Ch 11 HW Resources A student needs to dilute a 0.35 M Pb(NO), solution to make 93.0 mL of 0.15 M Pb(NOG), Set up the calculation by placing the values with the correct units into the equation. Then, calculate the volume, in milliliters, of the 0.35 M Pb(NO), solution that is needed. Answer Funk 0.35 ml 0.35 M 0.15 M
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
A chemist must dilute 64.5 ml of 3.43 M aqueous Calcium bromide (CaBr) solution until the concentration fails to 3.00 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. Be sure your answer has the correct number of significant digits. X 5 ?
You wish to make a 0.249 M hydrobromic acid solution from a stock solution of 12.0 M hydrobromic acid. How much concentrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? __mL You wish to make a 0.112 M nitric acid solution from a stock solution of 12.0 M nitric acid. How much concentrated acid must you add to obtain a total volume of 150 mL of the dilute solution? __mL In the...
A student pipets 5.00 mL of a 5.103 M aqueous NaOH solution into a 250.00 mL volumetric flask and dilutes up to the mark with distilled water. What is the final molarity of the dilute solution? Select one: A. 0.1 MX B. 0.10206 M C. 0.102 M D. 0.1021 M Your answer is incorrect. 86.14 mL of an acid solution was needed to neutralize 30.24 mL of a base solution of unknown concentrations. A second trial is run but this...
To what volume should you dilute 132 mL of an 8.05 M CuCl2 solution so that 49.0 mL of the diluted solution contains 4.45 g CuCl2? Express your answer in milliliters.
To what volume should you dilute 128 mL of an 8.10 M CuCl2 solution so that 49.0 mL of the diluted solution contains 4.77 g CuCl2? Express your answer in milliliters.
14. 35.00 mL of a 0.30 M HCl solution is titrated with 0.35 M NaOH. What is the pll of the solution after 28.00 mL of the NaOH has been added? (show your calculation steps) - 15. How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 x 10-8. (show your calculation steps)