Concept explainers
(a)
Interpretation:
The concentration of
(a)
Answer to Problem 137QRT
The concentration of
Explanation of Solution
Given information is given as,
As known,
So,
Conversion of ppm to ppb as follows,
Hence, the concentration of
(b)
Interpretation:
The molarity of
(b)
Answer to Problem 137QRT
The molarity of
Explanation of Solution
A sample of exactly
Hence, molarity of
(c)
Interpretation:
From one metric ton of cassiterite, number of
(c)
Answer to Problem 137QRT
The number of bottles calculated as
Explanation of Solution
The given reaction;
In exactly one metric ton,
So, the actual mass of Tin is,
The theoretical mass of
The actual mass of
Number of bottles is calculated by using bottle volume; which is calculated by molarity obtained
Hence, number of bottles calculated as is
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Chapter 13 Solutions
Chemistry: The Molecular Science
- Assume that a sample of hard water contains 50. mg/L of Mg2+ and 150 mg/L of Ca2+, with HCO3 as the accompanying anion. What mass of CaO should be added to 1.0 L of this aqueous solution to precipitate all the Mg2+ and Ca2+ as CaCO3 and MgCO3? What is the total mass of the two solids formed?arrow_forwardFluoridation of city water supplies has been practiced in the United States for several decades. It is done by continuously adding sodium fluoride to water as it comes from a reservoir. Assume you live in a medium-sized city of 150,000 people and that 660 L (170 gal) of water is used per person per day. What mass of sodium fluoride (in kilograms) must be added to the water supply each year (365 days) to have the required fluoride concentration of 1 ppm (part per million)that is, 1 kilogram of fluoride per 1 million kilograms of water? (Sodium fluoride is 45.0% fluoride, and water has a density of 1.00 g/cm3.)arrow_forward148. Addition of 50.00 mL of 2.238 m H2SO4 (solution density = 1.1243 g/mL) to 50.00 mL of 2.238 M BaCl2 gives a white precipitate. (a) What is the mass of the precipitate in grams? (b) If you filter the mixture and add more H2SO4 solution to the filtrate, would you obtain more precipitate? Explain.arrow_forward
- 25. Which of the following has maximum solubility at low pH? (a) NH,CI (c) Na,PO4 (b) NaCl (d) Sr(OH),arrow_forward(a) Write chemical equations to show what happens when each of the following substances is mixedwith water:(i) Hydride ion(ii) Glucose, C6H12O6(s)(iii) Copper(II) bromide(iv) Formic acid(b) Write chemical equations for the following processes:(i) Chemical reaction for ΔH°f for mercury(I) phosphate.(ii) Thermal dissociation of gaseous bromine.(iii) Sublimation of carbon dioxide.(iv) Reduction of VO2+ to produce VO2+.(v) Neutralization of sulfuric acid by barium hydroxide.(vi) Thermal decomposition of 1 mol of sodium bicarbonate to produce sodium carbonate, carbon dioxide and waterarrow_forwardCopper(I) ions in aqueous solution react with NH3(aq) according to Cu^+ (aq) + 2NH3 ----> Cu(NH3)2 ^+(aq) Kf= 6.3*10^10 Calculate the solubility (in g·L–1) of CuBr(s) (Ksp = 6.3× 10–9) in 0.26 M NH3(aq). solubility of CuBr(s): g/Larrow_forward
- A student wants to dissolve the maximum amount of CaF₂(Kₛₚ=3.2X10⁻¹¹) to make 1 L of aqueous solution.(a) Into which of the following solvents should she dissolve the salt?(I) Pure water(II) 0.01 M HF (III) 0.01 M NaOH(IV) 0.01 M HCl(V) 0.01 M Ca(OH)₂ b) Which would dissolve the least amount of salt?arrow_forwardThe thermodynamic solubility product of A9CN is 6.0×10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.75e-9 mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.81e-16 X mol·L-1arrow_forward(5) A titration is setup so that NaOH is in a buret and 25.0 mL of HBr soln is in a flask. The NaOH has a known molarity of 0.250 M. At the end point 36.3 mL of NaOH has been added to the HBr soln. What is the molarity of the HBr? (6) A second titration is performed using the same 0.250 M NaOH in a buret. This time 25.0 mL of an H2S04 soln is titrated. At the endpoint 47.8 mL of NaOH has been added to the H2SO4 soln. What is the molarity of the H2S04? 4arrow_forward
- Describe the changes in pH that take place during the titration of: (a) a weak acid with a strong base, (b) a weak base with a strong acid .arrow_forwardThe solubility of Cr(NO3)3 . 9 H2O in water is 208 g per 100 gof water at 15 °C. A solution of Cr(NO3)3 # 9 H2O in water at35 °C is formed by dissolving 324 g in 100 g of water. Whenthis solution is slowly cooled to 15 °C, no precipitate forms.(a) Is the solution that has cooled down to 15 °C unsaturated,saturated, or supersaturated? (b) You take a metal spatulaand scratch the side of the glass vessel that contains thiscooled solution, and crystals start to appear. What has justhappened? (c) At equilibrium, what mass of crystals do youexpect to form?arrow_forward2. What is the solubility of magnesium sulfate in terms of molality if K= 1.08×10° in: (a) pure water? (b) an aqueous solution with an ionic strength of 0.0020?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning