1.
In the laboratory, a student dilutes 27.6 mL of a 10.2 M hydrobromic acid solution to a total volume of 150.0 mL. What is the concentration of the diluted solution?
Concentration = ______M
How many milliliters of 11.8 M hydrobromic acid solution should be used to prepare 2.50 L of 0.400 M HBr?
______mL
2.
In the laboratory a student combines 41.2 mL of
a 0.440 M cobalt(II) acetate
solution with 23.1 mL of a 0.311
M lead acetate solution.
What is the final concentration of acetate anion
?
______ M
In the laboratory a student combines 38.5 mL of
a 0.379 M calcium chloride
solution with 20.1 mL of a 0.652
M calcium iodide solution.
What is the final concentration of calcium cation
?
_____ M
1. In the laboratory, a student dilutes 27.6 mL of a 10.2 M hydrobromic acid solution...
In the laboratory, a student dilutes 15.1 mL of a 7.96 M hydrobromic acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution?
Part A. In the laboratory, a student dilutes 13.1 mL of a 7.41 M hydrochloric acid solution to a total volume of 250.0 mL. What is the concentration of the diluted solution? Concentration = M Part B. How many milliliters of 8.57 M hydrobromic acid solution should be used to prepare 4.00 L of 0.400 HBr M ? mL
In the laboratory a student combines 46.5 mL of a 0.347 M potassium iodide solution with 27.7 mL of a 0.379 M potassium acetate solution. What is the final concentration of potassium cation? M
In the laboratory, a student dilutes 10.5 mL of a 6.50 M nitric acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution? Concentration = M.
In the laboratory, a student dilutes 10.3 mL of a 11.5 M perchloric acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution? Concentration = ?? M
In the laboratory, a student dilutes 22.7 mL of a 6.53 M perchloric acid solution to a total volume of 200.0 mL. What is the concentration of the diluted solution? Concentration = ___M
please answer the following question In the laboratory, a student dilutes 28.4 mL of a 8.32 M hydrobromic acid solution to a total volume of 100.0 mL. What is the concentration of the diluted solution? Concentration = M
1a. In the laboratory a student combines 33.0 mL of a 0.315 M zinc fluoride solution with 22.9 mL of a 0.620 M zinc chloridesolution. b. What is the final concentration of zinc cation ? 2a. In the laboratory a student combines 26.5 mL of a 0.383 M barium bromide solution with 10.3 mL of a 0.448 M calcium bromide solution. b. What is the final concentration of bromide anion ?
1) In the laboratory a student combines 35.3 mL of a 0.376 M potassium bromide solution with 26.6 mL of a 0.595 M potassium sulfate solution. What is the final concentration of potassium cation ? M 2) In the laboratory a student combines 43.3 mL of a 0.438 M iron(III) bromide solution with 21.7 mL of a 0.303 M aluminum bromide solution. What is the final concentration of bromide anion ? M 3)In the laboratory a student combines 20.0 mL...
In the laboratory, a student dilutes 26.4 mL of a 10.5 M nitric acid solution to a total volume of 250.0 mL. What is the concentration of the diluted solution? Concentration = How many milliliters of 11.6 M hydrochloric acid solution should be used to prepare 5.50 L of 0.100 M HCl? Interpret the following equation for a chemical reaction using the coefficients given: CO(g) + Cl2(g) →→ COC12(g) On the particulate level: of CO(g) reacts with — of Cl2(g)...