Part 3: Solution Stoichiometry (section 9.4)1. A 10.0 mL sample of an unknown H3PO4 solution requires 112 mL of 0.100 M KOHto completely react with the H3PO.. What is the molarity (M) of the unknown H&POsolution? (Identify 'given' and 'needed quantities and set up a plan to solve theproblem).НаРОд (аq) + ЗКОН (аq)KЗРОa (аq) + 3Н20 (1)

Given, Volume of H3PO4 = 10.0 mL Molarity of KOH = 0.100M Volume of KOH = 112mL

Part 3: Solution Stoichiometry (section 9.4) 1. A 10.0 mL sample of an unknown H3PO4 solution requires 112 mL of 0.100 M KOH to completely react with the H3PO4. What is the molarity (M) of the unknown HoPO solution? (Identify 'given' and 'needed' quantities and set up a plan to solve the problem). НЭРО4 (аq) + ЗКОН (аq) KPO4 (aq) + 3H2O (I)

Part 3: Solution Stoichiometry (section 9.4) 1. A 10.0 mL sample of an unknown H3PO4 solution requires 112 mL of 0.100 M KOH to completely react with the H3PO4. What is the molarity (M) of the unknown HoPO solution? (Identify 'given' and 'needed' quantities and set up a plan to solve the problem). НЭРО4 (аq) + ЗКОН (аq) KPO4 (aq) + 3H2O (I)

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

2. A solution of ethanol (d = 0.795 g/mL) and water (H,O) is prepared by placing 30.0 mL of ethanol in a 250.0 mL volumetric flask and diluting with water to the flask etched mark. %3D a. What is the molarity of the ethanol in this solution?
An aqueous potassium iodate stock solution is made by dissolving 7.39 mol KIO, in sufficient water for the final volume of the solution to be 4.00 L. Calculate the molarity of the stock KIO, solution. molarity of stock KIO, solution= M A 10.0 mL aliquot is removed from the described stock solution and diluted to a total volume of 100.0 mL. Calculate the molarity of the dilute solution. M molarity of dilute KIO, solution=
Consider the reaction: 2 NaBH4(aq) + H₂SO4(aq) → 2 H₂(g) + Na₂SO4(aq) + B₂H6(9) What volume, in mL, of a 0.529 M solution of NaBH4 is required to produce 0.591 g of B₂H6? H₂SO4 is present in excess. mL Submit The desired mass of the product, B₂H6, is 0.591 g. What is this amount of B₂H5, in units of moles? mol B₂H6 Submit
What’s the answer in g
An aqueous solution is made by dissolving 45.0 g of H2SO4in 850. g of water. The density of water is 1.00 g/mL A) What is the concentration of the starting solution in percent by mass (%m/m)? B) What is the molarity of the H2SO4solution? C) If 25.0 mL of this solution is diluted to 500. mL, what is the resulting molarity?
Tin(IV) sulfide, SnS2, a yellow pigment, can be produced using the following reaction. SnBr4(aq)+2Na2S(aq)⟶4NaBr(aq)+SnS2(s) Suppose a student adds 46.6 mL of a 0.600 M solution of SnBr4 to 51.4 mL of a 0.154 M solution of Na2S. 1) Calculate the theoretical yield of SnS2 (in grams) 2) The student recovers 0.386 g of SnS2. Calculate the percent yield of SnS2 that the student obtained.
<3 of 110 A B assroom.collegeboard.org C D A student obtains 500. mL of a 1.0 M solution of NaCl(aq). Which of the following changes would result in a solution with a final molarity that is closest to 2.0 M ? OX 4042% 11:46 Dissolving 15 g of NaCl in the solution Dissolving 29 g of NaCl in the solution Pouring out 250. mL of the solution Adding 500. mL of water to the solution Submit :D : = f(x)
3. What is the mass percent of a solution made by adding 22.3 g of NaOH to 100.0 g of wa = 22.39 Na0H 22.39 NaOlt + [009 A20 x lou 18.2% 4. How many grams of water must be added to 15.0 g NaCl to make a solution that is 10.0%(m/m)? What is the molarity of a 50.0% by mass solution of nitric acid? (Density=2.5 I
Granulated sugar (sucrose, C12H22O11) has an average density of about 0.70 g/cm3. Calculate the molarity of sucrose if 2.0 tsp of sugar is added to a 8.0 oz cup of coffee. 1.00 tsp = 4.93 cm3
in the conversion to biodiesel, the Jojoba oil is reacted in a 1.0M solution of sodium methoxide in methanol. A simple way to prepare this solution is to treat methanol with solid sodium metal, which reacts to generate sodium methoxide by the following equation: 2Na(s) + 2CH30H -> 2Na+ + 2CH30 + H2(g) What mass of solid sodium metal should be added to 500mL of methanol to generate a 1.0M NaOMe solution? 11.50g O 5.75g 23.00g 22.99g O 0.12g
What mass of sodium hydroxide (NaOH, molar mass = 40.0 g∙mol–1) is needed to make 100.0 mL of a 0.125 M NaOH solution?
3. How many grams of NaOH are needed to prepare 45.0 mL of a 6.00 M solution? 4. What is the molar concentration of 17.5% (v/v) aqueous solution of hydrochloric acid? The density of hydrochloric acid is 1.49 g/mL. Assume the solution is 100.00 mL. 5. What is the concentration of a solution of H₂SO4 if 95.0 mL of a 2.50 M H₂SO4 solution is diluted to a total volume of 275.0 mL? 6. What volume of a 2.28 M aqueous sodium carbonate will completely react with 125 mL of 0.525 M aqueous calcium chloride? 7. 100.0 mL of 0.445 M potassium hydroxide is mixed with 90.0 mL of 0.215 M magnesium nitrate. a. Write the net ionic equation. b. Find the mass of the precipitate in the solution. | c. How many moles of excess reagent will remain at the end of the reaction?