Solution Stoichiometry

Manganese in an ore can be determined by treating the ore with a measured, excess quantity of sodium oxalate (Na2C2O4) to reduce MnO2(s) to MnCl 2(aq) followed by determination of the unreacted sodium oxalate by titration with potassium permanganate. The equations for this two step process are:   MnO2(s) + Na2C2O4(aq) + 4HCl(aq) → 2MnCl 2(aq) + 2CO2(g) + 2H2O(l) +2NaCl(aq)   2KMnO4(aq) + 5Na2C2O4(aq) + 16HCl(aq) → 2MnCl 2(aq) + 10CO2(g) + 8H2O(l) + 10NaCl(aq)   If a sample is treated with 50.0 mL of 0.275 M Na 2C2O4(aq) and the unreacted Na 2C2O4(aq) requires 18.28 mL of 0.1232 M KMnO4(aq), calculate the number of grams of manganese in the sample. (NOTE: use the equations as written despite the fact they are not completely balanced) 

Consider the following reaction sequence for the determination of dissolved oxygen in water:   2MnSO4(aq) + 4NaOH(aq) + O 2(aq) → 2MnO2(s) + 2Na2SO4(aq) + 2H2O(l) MnO2(s) + 2H2SO4(aq) + 2NaI(aq) → MnSO 4(aq) + I 2(aq) + Na 2SO4(aq) + 2H 2O(l) I2(aq) + 2Na 2S2O3(aq) → Na 2S4O6(aq) + 2NaI(aq)   If 9.00 mL of 0.0240 M Na 2S2O3(aq) are used in the analysis, how many moles of dissolved oxygen were determined? a) 4.32 x 10-4 mol b) 2.70 x 10-5 mol c) 5.40 x 10-5 mol d) 2.16 x 10-4 mol e) 1.08 x 10-4 mol 

The iron content in ores can be determined by titrating a sample with a solution of potassium permanganate. The ore is first dissolved in hydrochloric acid, forming iron (II) ions, which react with permanganate ions according to the following net-ionic reaction: MnO4- (aq) + 5 Fe 2+ + 8H + (aq) → Mn 2+ (aq) + 5 Fe 3+ (aq) + 4 H 2O (l) A sample of ore of mass 0.202g was dissolved in hydrochloric acid, and the resulting solution needed 16.7 mL of 0.0108 M KMnO4(aq) to reach the stoichiometric point. What mass of iron (II) ions are present?         What is the mass percentage of iron in the sample of ore?

A 55.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead (II) acetate solution and this precipitation reaction occurs: K2SO4 (aq) + Pb(C2H3O2)2 (aq)      →       2 KC 2H3O2 (aq) + PbSO4 (s) The solid PbSO4 is collected , dried, and found to have a mass of 1.01 g. Determine the limiting reactant, the theoretical yield, and the percent yield. 

What volume (in mL) of 0.500 M KMnO 4 is required to react with 0.2506 g of Cu+ according to the equation: MnO4– + 5 Cu+ + 8 H+      ⇌       Mn2+ + 4H2O    a) 1.58 b) 15.8 c) 7.9 d) 0.176 e) 0.100

What volume of a 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution to the reaction below?   2 KCl (aq) + Pb(NO 3)2 (aq) → PbCl2 (s) + 2 KNO 3 (aq)   a. 97.4 mL b. 116 mL c. 43.0 mL d. 86.1 mL e. 58.1 mL

In the following redox reaction, dichromate ion, Cr 2O7 2- , oxidizes Fe2+ to yield the following products. Cr2O7 2- (aq) + 6 Fe 2+ (aq) + 14 H + (aq) → 2 Cr 3+ (aq) + 6 Fe 3+ (aq) + 7 H 2O (l) If it takes 35.0 mL of 0.250 M FeCl 2 to titrate 100 mL of a solution containing Cr 2O7 2- , what is the molar concentration of Cr2O7 2- ?  a. 0.015 M b. 0.053 M c. 0.027 M d. 0.045 M

Iron (III) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation below. How many microliters of a 0.250 M FeCl2 are needed to completely react with 8.24 g of a compound containing 31.3% weight K2Cr2O7?   Cr2O7 2- + 6 Fe 2+ + 14 H+ → 2 Cr3+ + 6 Fe 3+ + 7 H2O

What volume of 0.131 M BaCl 2 is required to react completely with 42.0 mL of 0.453 M Na2SO4? The following is the net ionic equation. Ba2+ (aq) + SO42- (aq) → BaSO4(s) A. 12.1 mL B. 72.6 mL C. 145 mL D. 290 mL

Calculate the number of moles of iron(III)sulfide that forms when 62.0 mL of 0.135 M iron(III)chloride reacts with 45.0 mL of 0.285 M calcium sulfide. a) 8.56 x 10−3 mol b) 4.19 x 10−3 mol c) 1.25 x 10−2 mol d) 4.28 x 10−3 mol e) 8.38 x 10−3 mol

In acidic solution, the dichromate ion, Cr2O72– (aq) will oxidize Fe2+ to Fe3+ and form Cr3+. This net ionic equation represents the reaction that takes place during the reaction.  Cr2O72- (aq) + 6 Fe2+ (aq) + 14H+(aq) → 2 Cr3+ (aq) +6Fe3+ (aq) + 7 H2O(l) What volume of 0.100 M Cr 2O7 2- (aq) is required to oxidize 60.0 mL of 0.250 M Fe 2+(aq)? a) 25.0 mL b) 42.0 mL c) 58.4 mL d) 175 mL

What volume of 0.131 M BaCl2 is required to react completely with 42.0 mL of 0.453 M Na2SO4? This is the net ionic equation for the reaction. Ba2+(aq) + SO42-(aq) → BaSO4(s) a) 12.1 mL b) 72.6 mL c) 145 mL d) 290 mL

Sulfuric acid cannot be stored in an aluminum container because sulfuric acid dissolves aluminum metal. The following equation shows the reaction: 2 Al (s) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 3 H2 (g) Calculate the volume of sulfuric acid that would be required to completely dissolve a 4.643 g block of aluminum if you are given a 0.98 M H2SO4 solution. A. 175.60 mL B. 710.66 mL C. 284.48 mL D. 263.40 mL E. 242.33 mL  

 How many moles of AgCl are formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl 2 solution? 2 AgC2H3O2 (aq) + MgCl 2 (aq) → 2 AgCl (s) + Mg(C2H3O2)2 (aq) a. 0.0120 moles AgCl b. 0.0117 moles AgCl c. 0.00585 moles AgCl d. 0.0600 moles AgCl

Consider the following balanced redox equation:  H2O  +  2 MnO4 –  +  3 SO32- →   2 MnO2  +  3 SO42-  +  2 OH – a)  How many moles of SO32- (MW:80.07 g/mol) are required to completely react with 20.3 mL of a 0.500 M MnO4– (MW: 118.90 g/mol) solution? a. 0.0152 moles SO32- b. 0.0067 moles SO32- c. 0.005075 moles SO32- d. 0.3045 moles SO32-     b) How many mL of a 1.25 M Na 2SO3 (MW: 126 g/mol) are required to completely react with 2.55 mL of a 3.50 M KMnO4 (MW: 158 g/mol) solution?            c) How many grams of MnO 2 (MW: 86.94 g/mol) are produced when 32.0 mL of 0.615 M MnO 4- (MW: 118.90 g/mol) reacts with excess water and sulfite?   

Blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium dichromate, K2Cr2O7, solution. The balanced redox equation is given below: H+ (aq) + 2 Cr2O72- (aq) + C2H5OH (aq) → 4 Cr3+ (aq) + 2 CO 2 (g) + 11 H2O (l) If 45.12 mL of 0.04918 M Cr 2O72- solution is required to titrate 25.0 mL of C 2H5OH, what is the molar concentration of C2H5OH? a. 0.05450 M b. 0.01362 M c. 0.17752 M d. 0.04438 M

According to the following balanced reaction, how many moles of Fe(OH) 2 can form from 175.0 mL of 0.227 M LiOH solution?  Assume that there is excess FeCl2.              FeCl2(aq) + 2 LiOH(aq)  →  Fe(OH)2(s) + 2 LiCl(aq) A) 3.97 × 10−2 moles B) 2.52 × 10−2 moles C) 1.99 × 10−2 moles D) 5.03 × 10−2 moles E) 6.49 × 10−2 moles

The SO2 present in air is mainly responsible for the acid rain phenomenon. Its concentration can be determined by titrating against a standard permanganate solution as follows: 5 SO2 + 2 MnO4- + 2 H2O → 5 SO42- + 2 Mn2+ + 4 H+ Calculate the number of grams of SO 2 in a sample of air if 7.37 mL of 0.00800 M KMnO 4 solution are required for the titration.

A 0.250 M solution of sulfuric acid (H2SO4) is to be reacted with a solution of sodium hydroxide via a double-displacement reaction to make sodium sulfate and water. 50.0 mL of the H2SO4 solution reacts with 25.0 mL of the NaOH solution. What is the molarity of the NaOH solution? (A) 0.0625 M (B) 0.125 M (C) 0.250 M (D) 0.500 M (E) 1.00 M

What volume of a 0.100 M HCl solution is required to exactly neutralize 25.0 mL of 0.235 M Ba(OH)2? The balanced equation is 2HCl(aq) + Ba(OH)2 → BaCl2 + 2H2O(l). a. 235 mL b. 117.5 mL c. 58.8 mL d. 29.4 mL e. 1.18 x 103 mL

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? 

What is the molar mass of a 0.350 g sample of a monoprotic acid if it requires 50.0 mL of 0.440 M Ca(OH)2 to completely neutralize it? 

What volume (L) of a 2.50 M SrCl2 will completely react with 0.150 L of a 1.75 M AgNO3 solution?SrCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Sr(NO3)2(aq)A. 0.0525 LB. 0.210 LC. 0.0686 LD. 0.429 L

How many mL of 0.200 M H2SO4 (aq) must be added to 25.0 mL of 0.0888 M BaCl2 (aq) to precipitate all the barium as barium sulfate?a) 22.2 mLb) 25.0 mLc) 9.01 mLd) 5.55 mLe) 11.1 mL

It requires 23.56 mL of 0.105 M sodium hydroxide to neutralize 15.00 mL of a sulfuric acid (H2SO4) solution. Determine the concentration of the sulfuric acid (H2SO4) solution.       The titration of 25.0 mL of an H 2SO4 solution of unknown concentration requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution?

A 25.0 mL sample of 0.15 M silver nitrate, AgNO 3, is reacted with a 3.58 g sample of calcium chloride, CaCl2, (M= 111.0). Which of the following statements is true? a) Silver nitrate is the limiting reactant and calcium nitrate precipitates. b) Silver nitrate is the limiting reactant and silver chloride precipitates. c) Calcium chloride is the limiting reactant and calcium nitrate precipitates. d) Calcium chloride is the limiting reactant and silver chloride precipitates.

30.mL of 0.10 M Ca(NO3)2 and 15.0 mL of 0.20 M Na 3PO4 solutions are mixed. After the reaction is complete, which of these ions has the lowest concentration in the final solution?a) Na+b) NO3–c) Ca2+d) PO43–

ln an acid-base titration, a 20.0 mL HCI solution of unknown concentration requires 15.6 mL of a 0.250 M NaOH solution to reach the equivalence point. What is the concentration (M) of the unknown HCI solution? HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq)A. 12.1 MB. 72.6 MC. 320 MD. 0.195 M

What mass of KCl is needed to precipitate the silver ions from 15.0 mL of 0.200 M AgNO3 solution?

What mass of NaOH is needed to precipitate the Cd  2+ ions from 35.0 mL of 0.500 M Cd(NO3)2 solution?

(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution?

(b) How many milliliters of 0.125 M H 2SO4 are needed to neutralize 0.200 g of NaOH?

Calculate the molarity of each of these solutions.c. A 0.1025-g sample of copper metal is dissolved in 35 mL of concentrated HNO 3 to form Cu2+ ions and then water is added to make a total volume of 200.0 mL. (Calculate the molarity of Cu2+.)

What mass of Na2CrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100 M solution of AgNO3?

What volume of 0.100 M Na3PO4 is required to precipitate all the lead(II) ions from 150.0 mL of 0.250 M Pb(NO3)2?

What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?

What mass of barium sulfate can be produced when 100.0 mL of a 0.100 M solution of barium chloride is mixed with 100.0 mL of a 0.100 M solution of iron(III) sulfate?

What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO 3 is added to 20.0 mL of 1.00 M NaBr?

You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.c. Calculate the percent sodium chloride in the original unknown mixture.

What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?a. 0.100 M NaOH

What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?b. 0.0500 M Ba(OH)2

What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?b. 0.0500 M Sr(OH)2

What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?c. 0.250 M KOH

A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?

A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.a. What is the molarity of the acetic acid?

A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.b. If the density of the vinegar is 1.006 g/cm 3, what is the mass percent of acetic acid in the vinegar?

What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?

A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.

A student titrates an unknown amount of potassium hydrogen phthalate (KHC 8H4O4, often abbreviated KHP) with 20.46 mL of a 0.1000 M NaOH solution. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

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, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.

Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with 3.210 g of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 5.0 M HCl is required to react completely with 3.00 g of magnesium?

Douglasite is a mineral with the formula 2KCl • FeCl 2 • 2H2O. Calculate the mass percent of douglasite in a 455.0-mg sample if it took 37.20 mL of a 0.1000 M AgNO3 solution to precipitate all the Cl– as AgCl. Assume the douglasite is the only source of chloride ion.

A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?

What volume of 0.0521 M Ba(OH) 2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4? Phosphoric acid contains three acidic hydrogens.

A 10.00-mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? Sulfuric acid contains two acidic hydrogens.

A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH– ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.

A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete reaction. Determine the molar mass of the acid.

Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?

Determine the number of grams of H 2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 x 1023 atoms of Fe according to the following reaction.2 HCl(aq) + Fe(s) → H 2(g) + FeCl 2(aq)A) 0.374 gB) 1.33 gC) 1.14 gD) 0.187 gE) 1.51 g

How much 0.5685 M nitric acid, HNO 3, solution would a student need to use to neutralize 0.8232 g of Al(OH)3?a. 37.12 mLb. 18.56 mLc. 32.92 mLd. 55.69 mLe.47.48 mL

Vinegar is a solution of acetic acid, CH 3COOH, dissolved in water. A 5.54 g sample of vinegar was neutralized by 30.10 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar?a) 24.4 %b) 0.109 %c) 3.26 %d) 9.79 %

What is the molar mass of a 0.350 g sample of a monoprotic acid if it requires 50.0 mL of 0.440 M Ca(OH)2 to completely neutralize it? a) 5.30 g/molb) 7.95 g/molc) 31.8 g/mold) 47.7 g/mol

We use 625. mL of a sodium hydroxide, NaOH, solution to completely neutralize 4.50 grams of phosphoric acid.a. What is the molarity of the NaOH solution?    b. What are the name and the mass of the salt that forms?

What volume of 0.405 M KOH solution is needed to react completely with 2.15 g of copper (II) sulfate, CuSO4? The products of the chemical reaction are copper (II) hydroxide and potassium sulfate.

Given the precipitation of AgCl from a NaCl solution using silver nitrate:AgNO3 + NaCl(aq) →  AgCl(s) + NaNO3(aq)If a solution of AgNO3 of unknown molarity is added to a flask containing 132ml of NaCl solution also of unknown molarity. At the endpoint 42.15 ml of the AgNO3 solution have been added and 8.42 g of AgCl are recovered as a precipitate from the reaction:a) What is the molarity of the NaCl solution?  b) What is the molarity of AgNO3 solution? 

What volume of 3.05 M HCl(aq) will react with 25.0 g Zn(s)? Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)a. 0.251 Lb. 4.01 Lc. 0.125 Ld. 0.0627 Le. 2.33 L  

A solution of hydrochloric acid is to be neutralized by using a 0.15 M solution of barium hydroxide. 25.0 mL of the HCl solution requires 33.3 mL of the Ba(OH)2 solution. What is the molarity of the HCl solution?A. 0.40 MB. 0.11 MC. 0.15 MD. 0.20 ME. 0.22 M

How many grams of barium phosphate (molar mass= 601.93 g ) are produced by mixing 209.28 mL of 0.182 M barium nitrate with 127.80 mL of 0.173 M sodium phosphate?  3Ba(NO3)2 + 2Na 3PO4 → Ba3(PO4)2 + 6NaNO3A) 7.64 gramsB) 13.3 gramsC) 6.65 gramsD) 4.44 gramsE) 22.9 grams

Calculate the amount, in mL, of 0.0168 M Ca(OH) 2 that would be required to completely react with 25.38 mL of 0.0784 M HClO3.A) 5.44 mLB) 59.22 mLC) 236.88 mLD) 2.72 mLE) 10.88 mL

Sodium hydrogen carbonate (NaHCO 3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCl), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction:HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H 2O (I) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution.Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50 mL of a 0.034 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.

When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation.     2AgNO3(aq)+MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)a) What mass of silver chloride can be producd from 1.49L of a 0.254M solution of silver nitrate?b) The reaction described in Part A required 4.00L of magnesium chloride. What is the concentration of this magnesium chloride solution?

What is the molarity of a NaOH solution if 23.6 mL are needed to titrate a 0.5116g sample of KHP?

Solid calcium bicarbonate (Ca(HCO3)2) reacts with aqueous hydrochloric acid (HCl) to form aqueous calcium chloride, liquid water, and carbon dioxide gas.What is the minimum amount of 0.2102 M hydrochloric acid (in milliliters) required to completely react with 8.362 g calcium bicarbonate?

Zinc reacts with hydrochloric acid according to the reaction equation:Zn(s) + 2HCl(aq) → ZnCl 2(aq) + H2(g)How many milliliters of 2.50 M HCl(aq) are required to react with 8.15 g of Zn(s)?

Zinc reacts with hydrochloric acid according to the reaction equationZn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)How many milliliters of 6.00 M HCl(aq) are required to react with 5.65 g of Zn(s)?

Zinc reacts with hydrochloric acid according to the reaction equation:Zn + 2HCl → ZnCl2 + H2How many milliliters of 5.50 M HCl(aq) are required to react with 3.65 g of an ore containing 33.0% Zn(s) by mass?

A sample of CO32- antacid is dissolved with 25.0mL of 0.0981M HCl. The hydrochloric acid that is not neutralized by the antacid is titrated to a bromophenol endpoint with 5.83mL of 0.104M NaOH. Calculate the number of moles of base in the antacid.

The following equation is unbalanced.HNO3 + Ba(OH)2 → Ba(NO3)2 + H2OIf 12.0 mL of 0.600M of HNO3 solution reacts with 30.0 mL of 0.700M Ba(OH)2 solution, what is the molarity of Ba(OH)2 after the reaction is completed?

2HNO3(aq) + Ba(OH)2(aq) → 2H2O(l) + Ba(NO3)2(aq)0.1155 L sample of an unknown HNO3 solution required 42.9 mL of .10 M of Ba(OH) 2 for complete neutralization. What was the concentration of the HNO3 solution?

Pb(NO3)2 (aq) + 2NH4I(aq) → PbI2(s) + 2NH4NO3(aq)a) What volume of a 0.110 M NH4I solution is required to react with 923 mL of a 0.480 M Pb(NO 3)2 solution?b) How many moles of PbI2 are formed from this reaction?

20.0 mL of a 0.10 M solution of a diprotic acid (H 2A) are titrated with 0.20 M NaOH. How many mL of this NaOH solution are required to completely neutralize this acid solution?a. 25.0b. 20.0c. 15.0d. 10.0e. 5.00

Solid sodium hydroxide reacts with phosphoric acid according to the following equation: 3NaOH (s) + H3PO4 (aq) → Na 3PO4 (aq) + 3H 2O (l) What volume (in ml) of 0.0160 M phosphoric acid can be neutralized by 64.531 grams of sodium hydroxide? [molar masses: NaOH = 40.00 g/mole; H3PO4 = 98.00g/mole]

According to the following reaction, how many moles of Fe(OH) 2 can form from 175.0 mL of 0.2 M LiOH solution? Assume that there is excess FeCl2. FeCl2 (aq) + 2LiOH (aq) → Fe(OH) 2 (s) + 2LiCl (aq) a. 5.03 x 10- 2 moles b. 1.75 x 10 -2 moles c. 2.52 x 10 -2 moles d. 6.49 x 10 -2 moles e. 3.97 x 10 -2 moles

If 25.98 mL of 0.1180 M KOH solution reacts with 52.50 mL of CH 3COOH solution, what is the molarity of the acid solution?

A mordant is a substance that combines with a dye to produce a stable fixed color in a dyed fabric. Calcium acetate is used as a mordant. It is prepared by the reaction of acetic acid with calcium hydroxide.2CH3CO2 H + Ca(OH)2 ⟶ Ca(CH3CO2)2 + 2H2OWhat mass of Ca(OH)2 is required to react with the acetic acid in 25.0 mL of a solution having a density of 1.065 g/mL and containing 58.0% acetic acid by mass?

The reaction of  WCl6 with Al at ~400 °C gives black crystals of a compound containing only tungsten and chlorine. A sample of this compound, when reduced with hydrogen, gives 0.2232 g of tungsten metal and hydrogen chloride, which is absorbed in water. Titration of the hydrochloric acid thus produced requires 46.2 mL of 0.1051 M NaOH to reach the end point. What is the empirical formula of the black tungsten chloride?

Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titrations. If 19.15 mL of NaOH is required to neutralize 0.442 g of KHP, what is the concentration of NaOH?

The amount of I3- (aq) in a solution can be determined by titration with a solution containing a known concentration of S2O32- (aq) (thiosulfate ion). The determination is based on the net ionic equation 2 S2O32- (aq) + I3-(aq) → S4O62- (aq) + 3I-(aq) Given that it requires 30.4 mL of 0.470 M Na2S2O3 (aq) to titrate a 25.0-mL sample of I3- (aq), calculate the molarity of I3- (aq) in the solution. 

What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride is mixed with 100.0 mL of a 0.100-M solution of iron(III) sulfate?

How do you calculate the mass of KHC8H4O4 (molar mass=204.44 g/mol) that reacts with 15mL of 0.16 M NaOH solution ?

If 340 mL of 0.0824 M aqueous Ba 2+ and 230 mL of 0.253 M aqueous H + are reacted, how many mol of liquid H2O is produced?Ba(OH)2(aq) + 2HClO4(aq) → Ba(ClO4)2(aq) + 2H2O(l)

What is the molarity of ZnCl2 that forms when 30.0 g of zinc completely reacts with CuCl2 according to the following reaction? Assume a final volume of 285 mL.Zn(s) + CuCl2 (aq) → ZnCl2(aq) + Cu(s)

Lead(Il) nitrate and ammonium iodide react to form lead(Il) iodide and ammonium nitrate according to the Pb(NO3)2 (aq) + 2NH4I (aq) → PbI2 (s) + 2NH4NO3 (aq) a) What volume of a 0.370 M NH 4l solution is required to react with 429 mL of a 0.140 M Pb(NO3)2 solution? b) How many moles of Pbl2 are formed from this reaction?

Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to BaO2(s) + H2SO4(aq) → BaSO4(s) + H2O2(aq) How many milliliters of 3.00 M H2SO4(aq) are needed to react completely with 77.5 g of BaO2(s)?

Lead(ll) nitrate and ammonium iodide react to form lead(lI) iodide and ammonium nitrate according to the reaction Pb(NO3)2 (aq) + 2 NH4I (aq) →PbI2 (s) + 2 NH4NO3 (aq) What volume (mL) of a 0.270 M NH4I solution is required to react with 173 mL of a 0.460 M Pb(NO3)2 solution? How many moles of Pbl2 are formed from this reaction?

2 Al(NO3)3 + 3 Na 2CO3 → Al2(CO3)3 + 6 NaNO3Which product is precipitate?If 0.400 moles of aluminum nitrate is reacted with 0.700 moles of sodium carbonate, how many moles of precipitate will be formed? 

Calculate the mass in grams of MgCO3 precipitated by mixing 10.0 mL of a 0.200 M Na2CO3 solution with 5.00 mL of a 0.0500 M Mg(NO3)2 solution.