Interpretation:
The percentage of Vitamin C in the capsule should be determined.
Concept introduction:
Number of moles is equal to the ratio of given mass to the molar mass.
The mathematical expression is given by:
Number of moles =
Molarity is defined as the ratio of number of moles of solute to the volume of the solution in liters.
The mathematical expression is given by:
Molarity =
A solution of salt of metal when reacts with other solution to give products, the formula which is used to find the volume of either solution is given by:
Where, M1 and M2 are molarity of the solution
V1 and V2 are volume of the solution
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Chapter 4 Solutions
Chemistry: Principles and Reactions
- Oranges and grapefruits are known as citrus fruits because their acidity comes mainly from citric acid, H3C6H5O7. Calculate the concentration of citric acid in a solution if a 30.00-mL sample is neutralized by 15.10 mL of 0.0100 M KOH. Assume that three acidic hydrogens of each citric acid molecule are neutralized in the reaction.arrow_forwardGlycerol (C3H8O3) is commonly used as an additive to moisturizers. The amount of glycerol added can be determined by titration with permanganate in basic solution. 14MnO4(aq)+C3H8O3(aq)+20OH(aq)14MnO42(aq)+3CO32(aq)+14H2O How many milliliters of 6.15 M KMnO4 are required to completely react with 7.25 mL of an aqueous solution of glycerol (d=1.144g/mL) that is 51.6% by mass?arrow_forward1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does the reaction of Ba(OH)2(aq) + H+PO4(aq) fit? acid-base and oxidation-reduction oxidation-reduction acid-base and precipitation precipitationarrow_forward
- For a product to be called vinegar, it must contain at least 5.0% acetic acid, HC2H3O2, by mass. A 10.00-g sample of a raspberry vinegar is titrated with 0.1250 M Ba(OH)2 and required 37.50 mL for complete neutralization. Can the product be called a vinegar?arrow_forwardLactic acid, C3H6O3 is the acid present in sour milk. A 0.100-g sample of pure lactic acid requires 12.95 mL of 0.0857 M sodium hydroxide for complete reaction. How many moles of hydroxide ion are required to neutralize one mole of lactic acid?arrow_forwardAn antacid tablet contains sodium hydrogen carbonate, NaHCO3, and inert ingredients. A 0.465-g sample of powdered tablet was mixed with 53.3 mL of 0.190 M HCl (hydrochloric acid). The mixture was allowed to stand until it reacted. NaHCO3(s)+HCl(aq)NaCl(aq)+H2O(l)+CO2(g) The excess hydrochloric acid was titrated with 54.6 mL of 0.128 M NaOH (sodium hydroxide). HCl(aq)+NaOH(aq)NaCl(aq)+H2O(l) What is the percentage of sodium hydrogen carbonate in the antacid?arrow_forward
- Bone was dissolved in hydrochloric acid, giving 50.0 mL of solution containing calcium chloride, CaCL2. To precipitate the calcium ion from the resulting solution, an excess of potassium oxalate was added. The precipitate of calcium oxalate, CaC2O4, weighed 1.437 g. What was the molarity of CaCl2 in the solution?arrow_forwardThe active ingredients of an antacid tablet contained only magnesium hydroxide and aluminum hydroxide. Complete neutralization of a sample of the active ingredients required 48.5 mL of 0.187 M hydrochloric acid. The chloride salts from this neutralization were obtained by evaporation of the filtrate from the titration; they weighed 0. 4200 g. What was the percentage by mass of magnesium hydroxide in the active ingredients of the antacid tablet?arrow_forwardPotatoes can be peeled commercially by soaking them in a 3-M to 6-M solution of sodium hydroxide, then removing the loosened skins by spraying them with water. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to reach the end point?arrow_forward
- A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?arrow_forwardAn antacid tablet has calcium carbonate as the active ingredient; other ingredients include a starch binder. You dissolve the tablet in hydrochloric acid and filter off insoluble material. You add potassium oxalate to the filtrate (containing calcium ion) to precipitate calcium oxalate. If a tablet weighing 0.750 g gave 0.629 g of calcium oxalate, what is the mass percentage of active ingredient in the tablet?arrow_forwardChlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g sample of a medication containing the drug was treated to destroy the organic material and to release all the chlorine as chloride ion. When the filtered solution containing chloride ion was treated with an excess of silver nitrate, 0.104 g silver chloride was recovered. Calculate the mass percent of chlorisondamine chloride in the medication, assuming the drug is the only source of chloride.arrow_forward
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