5. A solution of calcium nitrate, (Ca(NO3)2, reacts with a solution of ammonium fluoride, NH4F, to form solid calcium fluoride, CaF2, and ammonium nitrate, NH&NO3 (aq). When 45.00 mL of 0.48724 M Ca(NO3)2 solution was added to 60.00 mL of 0.99981 M NH4F solution, 1.524 g of CaF2 was isolated from the filter paper. a. Write a balanced molecular equation for the reaction. Include all states of substances. b. Calculate the number of moles of product Ca(NO3)2 that you start with. C. Calculate the number of moles of NH4F that you start with. d. Calculate the grams of CaF2 that might be made based on your answers from 'b' & 'c' e. Identify the limiting reagent Ca(NO3)2 or NH&F (circle one) f. Calculate the percent yield of CaF2 based on the information given in the problem.

5. A solution of calcium nitrate, (Ca(NO3)2, reacts with a solution of ammonium fluoride, NH4F, to form solid calcium fluoride, CaF2, and ammonium nitrate, NH&NO3 (aq). When 45.00 mL of 0.48724 M Ca(NO3)2 solution was added to 60.00 mL of 0.99981 M NH4F solution, 1.524 g of CaF2 was isolated from the filter paper. a. Write a balanced molecular equation for the reaction. Include all states of substances. b. Calculate the number of moles of product Ca(NO3)2 that you start with. C. Calculate the number of moles of NH4F that you start with. d. Calculate the grams of CaF2 that might be made based on your answers from 'b' & 'c' e. Identify the limiting reagent Ca(NO3)2 or NH&F (circle one) f. Calculate the percent yield of CaF2 based on the information given in the problem.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

How many millilitres of 0.450 mol L−1 H2SO4(aq) are required to completely neutralize 46.7 mL of 0.930 mol L−1 KOH(aq) ? Hint: Write a balanced chemical equation for the reaction. Give your answer in mL, accurate to three significant figures. Do not include units as part of your answer.
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 53.0 mL of 0.461 M calcium nitrate?
A student needs to make 250 mL of 1.4 M Fe(NO3)3 by dilution. How many milliliters of a 5.0 M Fe(NO3)3 solution should the student use to prepare the solution?
6 ml of concentrated HCl acid solution was diluted to 180 mL. Then 65 mL sample of the diluted solution requires 18.8 mL of 0.3467 M NAOH solution for its titration. What is the molarity of the initial HCI solution?
3. Titration shows that a 5 mL sample of nitrous acid, HNO2, has a concentration of 0.5 M. If 8 mL of magnesium hydroxide, Mg(OH)2, were added to the acid to accomplish the neutralization, what must the molarity of the base have been?
1.45-g sample of oxalic acid, H2C2O4, is dissolved in distilled water to make 50.00 mL of aqueous solution. This solution is called “Solution A”. The 5.00 mL of Solution A is added to 20.00 mL of distilled water to make “Solution B”.H2C2O4(aq) reacts with MnO4–(aq) to produce CO2(g) and Mn2+(aq).When 19.41 mL of H2C2O4(aq) (Solution B) is mixed with 21.59 mL of 0.0400 M MnO4–(aq), the mass of CO2(g) obtained is 0.0990 g.(a) In this chemical reaction, which substance is the oxidizing agent? Why?(b) Calculate the percentage yield of CO2(g).(c) Determine the molarity of the excess reactant at the end of the chemical reaction.
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)₂(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.67 g PbCl₂ (s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)₂(aq) solution. concentration: M
Two solutions were made, the first one was made by dissolving 2.27 g of Co(NO3)2 in 100.0 mL of water. Then, to make the second solution, 5.00 mL of this solution was added to the 250 mL volumetric flask, which was filled to the mark with water. What was the molar concentration of the Co(NO3)2 in the two solutions?
In the neutralization of aqueous acetic acid with aqueous calcium hydroxide, 55.7 mL of 0.100 M Ca(OH)2 was required to react with 15.0 mL of CH3COOH. What was the molarity of the acetic acid solution?
250 mL of a 1.9 M Mg(OH)2 solution is added to a beaker. How many moles of Mg(OH)2 were added? How many grams of Mg(OH)2 were added?
16.792 g of Ba(OH)2 (171.342 g.mol') is weighed out and carefully dissolved to make a 500.00cm solution. A 25.00 cm of this solution is pipette then transfer into a 100.00 mL volumetric flask, filling up to the mark with water. A 40.00 mL sample of this diluted solution is then reacted with a 0.753 M solution of HNO3. Ba(OH)2(aq) + 2HNO3(aq) → Ba(N03)2(aq) + 2H2O(1) The concentration of Ba(OH)2 in the 100.00 cm3 volumetric flask is: O 1.96 x 103 M O 5.21 x 10-3 m O 4.90 x 10 2M O 1.96 x 101 M O 3.92 x 103 M O None of the above
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 48.82 mL of the sodium hydroxide solution was required to react with 0.7540 g KHP. Calculate the molarity of the sodium hydroxide. Molarity = ___________ M