sample of 5.93 g5.93 g of solid calcium hydroxide is added to 34.5 mL34.5 mL of 0.340 M0.340 M aqueous hydrochloric acid. Write the balanced chemical equation for the reaction. Physical states are optional. chemical equation:   What is the limiting reactant? a,calcium hydroxide b. hydrochloric acid   How many grams of salt are formed after the reaction is complete?   How many grams of the excess reactant remain after the reaction is

200. mL of 2.50 M H2SO4 is added to 300. mL of 4.00 M H2SO4. Assuming that the volumes are additive, what is the final concentration?

A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide to calcium oxide by heating. How many grams of calcium oxide should the student obtain if his solution contains 48.0 mL of 0.479 M calcium nitrate? g

6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)

Determine the limiting reactant and theoretical yield of the solid when 10.00 mL of a 1.00 M sodium sulfate solution is mixed with 18.00 mL of a 1.25M barium chloride solution to give solid barium sulfate and aqueous sodium chloride.

Consider the following serial dilution. A serial dilution is a stepwise dilution of a substance from a starting stock solution. Imagine you start with a 1.40 M stock solution and then take 59.0 mL of the stock solution and dilute it to a total volume of 238 mL. You then take a 119 mL aliquot of that solution and dilute it by adding 143 mL of water. What are the concentrations of the second and final solutions? Initial stock solution = Type your answer here M. Second solution = Type your answer here Final solution = Type your answer here Unanswered submit O Fullscreen 9:36 PM a 梦メ 4/25/2021 prt sc delete home end pg up 40 4. 6. num lock backspace 8. Y P. 7. home 个 pg K 4. enter G H. pause ↑ shift end |云 B

Calculate the molarity of each of these solutions.a. A 5.623-g sample of NaHCO3 is dissolved in enough water to make250.0 mL of solution.b. A 184.6-mg sample of K2Cr2O7 is dissolved in enough water to make500.0 mL of solution.c. A 0.1025-g sample of copper metal is dissolved in 35 Ml of concentrated HNO3 to form Cu2+ ions and then water is added to make a total volume of 200.0 mL. (Calculate the molarity of Cu2+.)

In an experiment, a student combines 75.0 mL of a 0.190 M iron (III) chloride solution with 125.0 mL of a 0.240 M sodium carbonate solution. a. Write a balanced equation for the reaction to see how many grams of sodium chloride need to be produced in the experiment in order to achieve a yield of 83.75%?

Consider a solution prepared by combining 45.0 g of BaCl2 with enough water to prepare a 750.0 mL of solution.  Assume that the volume of water added was 748 mL.  Density of water is 1.00 g/mL.  1)  What volume of this solution would be required to prepare 500.0 mL of a solution that is 0.0034 M in BaCl2?

2. 100.0 mL of 5.0 M Cu(NO3)2 was poured into a 1 L container. a. How many mols of Cu(NO3)2 is in the container? b. 350.0 mL of water was added. What is the concentration of NO3?