# 10 b-e 10. Use the equation below to calculate the following.1 Ca3(PO4)2 (s) + NaNO3 (aq)o aQ18 mot Naz POua. Balance the reaction. 3 Ca(NO3)2 (aq) + 2 NazPO4 (aq) →b. Moles of Na3PO4 needed to react with 1.45 L of 0.225M Ca(NO3)2c. Volume of 0.250 M Na3PO4 needed to react with 15.00 mL of 0.500 M Ca(NO3)2 do.Ome Nao Poud. Grams of Ca3(PO4)2 that can be obtained from 125 mL of 0.500 M Ca(NO3)2 u.Hua CaslPO4ne. Molarity of Ca(NO3)2 when 40.00 mL react with 50.00 mL of 2.00 M Na3PO4 25M Cs nw

The balanced reaction is given as, 3 Ca(NO3)2 (aq) + 2 Na3PO4 (aq) →Ca3(PO4)2 (s) + 6 NaNO3 (aq)

10. Use the equation below to calculate the follow 1 Ca3(PO4)2 (s) +_ NaNO3 (aq) a. Balance the reaction. 3 Ca(NO3)2 (aq) + 2 Na3PO4 (aq) b. Moles of Na;PO4 needed to react with 1.45 L of 0.225 M Ca(NO3)2 218 mot Naz PO, c. Volume of 0.250 M Na3PO4 needed to react with 15.00 mL of 0.500 M Ca(NO3)2 2o.Ome Ne Pou d. Grams of Caz(PO4)2 that can be obtained from 125 mL of 0.500 M Ca(NO3)2 u HUa CaslPO4)n e. Molarity of Ca(NO3)2 when 40.00 mL react with 50.00 mL of 2.00 M Na3PO4

10. Use the equation below to calculate the follow 1 Ca3(PO4)2 (s) +_ NaNO3 (aq) a. Balance the reaction. 3 Ca(NO3)2 (aq) + 2 Na3PO4 (aq) b. Moles of Na;PO4 needed to react with 1.45 L of 0.225 M Ca(NO3)2 218 mot Naz PO, c. Volume of 0.250 M Na3PO4 needed to react with 15.00 mL of 0.500 M Ca(NO3)2 2o.Ome Ne Pou d. Grams of Caz(PO4)2 that can be obtained from 125 mL of 0.500 M Ca(NO3)2 u HUa CaslPO4)n e. Molarity of Ca(NO3)2 when 40.00 mL react with 50.00 mL of 2.00 M Na3PO4

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter3: Molecules, Moles, And Chemical Equations

Section: Chapter Questions

Problem 3.61PAE: 3.61 Calculate the molarity of each of the following solutions. (a) 1.45 mol HCl in 250. mL of...

See similar textbooks

Similar questions

You are given a solid mixture of NaNO2 and NaCl and are asked to analyze it for the amount of NaNO2 present. To do so, you allow the mixture to react with sulfamic acid, HSO3NH2, in water according to the equation NaNO2(aq) + HSO3NH2(aq) NaHSO4(aq) + H2O() + N2(g) What is the weight percentage of NaNO2 in 1.232 g of the solid mixture if reaction with sulfa-mic acid produces 295 mL of dry N2 gas with a pressure of 713 mm Hg at 21.0 C?
When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
Twenty-five mL of a 0.388 M solution of Na2SO4 is mixed with 35.3 mL of 0.229 M Na2SO4. What is the molarity of the resulting solution? Assume that the volumes are additive.
Determine the volume of sodium hydroxide solution needed to prepare 26.2 g sodium phosphate, Na3PO4, by the reaction 3NaOH(aq)+H3PO4(aq)Na3PO4(aq)+3H2O(l) The sodium hydroxide solution, whose density is 1.133 g/mL, contains 12.0% NaOH by mass.
What is the molarity of a solution of sodium hydrogen sulfate that is prepared by dissolving 9.21 g NaHSO4 in enough water to form 2.00-L solution? What is the molarity of each ion in the solution?
Acetic acid (HC2H3O2) can be prepared by the action of the acetobacter organism on dilute solutions of ethanol (C2H5OH). The equation for the reaction is C2H5OH(aq)+O2(g)HC2H3O2(aq)+H2OHow many milliliters of a 12.5% (by volume) solution of ethanol are required to produce 175 mL of 0.664 M acetic acid? (Densityofpureethanol=0.789g/mL.)
A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.
Phosphoric acid is prepared by dissolving phosphorus(V) oxide, P4O10, in water. What is the balanced equation for this reaction? How many grams of P4O10 are required to make 1.19 L of aqueous solution containing 5.50% phosphoric acid by mass? The density of the solution is 1.025 g/mL.
A student wants to prepare 1.00 L of a 1.00-M solution of NaOH (molar mass = 40.00 g/mol). If solid NaOH is available, how would the student prepare this solution? If 2.00 M NaOH is available, how would the student prepare the solution? To help ensure three significant figures in the NaOH molarity, to how many significant figures should the volumes and mass be determined?
Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
4.49 Small quantities of hydrogen gas can be prepared by the following reaction: Zn(s)+H2SO4(aq)ZnSO4(aq)+H2(g) How many grams of H2 can be prepared from 25.0 mL of 6.00 M H2SO4 and excess zinc?
39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.