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Physical Chemistry
- Use the appropriate tables to calculate H for (a) the reaction between MgC03(s) and a strong acid to give Mg2+(aq), CO2(g), and water. (b) the precipitation of iron(III) hydroxide from the reaction between iron(III) and hydroxide ions.arrow_forwardCalcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?arrow_forwardThe following reaction occurs in pure water: H2O(l)+H2O(l)H3O+(aq)+OH-(aq) which is often abbreviated as H2O(l)H+(aq)+OH-(aq) For this reaction, G = 79.9 kJ/mol at 25C. Calculate the value of G for this reaction at 25C when [OH] = 0.15 M and [H+] = 0.71 M.arrow_forward
- A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.arrow_forwardSulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1=1x 10^3 and Ka2=1.2 x 10^(-2) .The initial concentration of sulphuric acid is given as 0.040M.Write the dissociation reactions. Calculate the concentration of [HSO4^- ] and [SO4^(2-)]. Calculate the pH of the acid solution. Write a discussion on the behaviour of polyprotic acids. (50 -100 words) Given: Ion product constant for water, Kw=1 x 10 ^(-14)arrow_forwardAluminum in the Al3 + form can be precipitated as Al (OH) 3, adding ammonia to an aluminum solution, but the precipitate is usually gelatinous and difficult to filter. Precipitation from a homogeneous solution provides a more filterable precipitate. The reaction used in this process is the hydrolysis of urea: (image attached) Suppose this reaction occurs in a 100.00 mL solution with an initial Al3 + concentration of 1.50x10-3 mol / L. How many moles of urea must be hydrolyzed to supply enough hydroxide to stoichiometrically combine Al3 + and form the precipitate Al (OH) 3?arrow_forward
- The solubility of strontium fluoride, SrF2, in moles per liter, can be expressed in terms of the resulting ion concentrations. Which relationship is correct? solubility=[F] O solubility=[2Sr²+] solubility=[Sr2+] solubility=2[Sr²+] solubility=2[F]arrow_forwardA 10.0 mL sample of 0.20 mol/L NiF2(aq) is mixed with 20.0 mL of 0.0700 mol/L NaOH(aq) and then diluted to a final volume of 100. mL. Calculate the concentration of OH- ions in the 100 mL mixture before the reaction starts. Express your answer to three significant figures.arrow_forwardk= 6.33 × 10−3 L·mol−1·s−1. If the initial concentration of XY is 0.150 mol·L−1, how long will it take for the concentration to decrease to 6.25 × 10−2 mol·L−1 ?arrow_forward
- a) Copper(I) ions in aqueous solution react with NH3(aq)NH3(aq) according to Cu+(aq)+2NH3(aq)⟶Cu(NH3)+2(aq)?f=6.3×10^10 Calculate the solubility (in g·L−1) of CuBr(s)CuBr(s) (?sp=6.3×10−9Ksp=6.3×10−9) in 0.19 M0.19 M NH3(aq)NH3(aq). solubility of CuBr(s)CuBr(s): g/L b) Given the equation Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)?f=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107 determine the concentration of NH3(aq) that is required to dissolve 589589 mg of AgCl(s) in 100.0 mL of solution. The ?spKsp of AgCl is 1.77×10−101.77×10−10. [NH3]= c) The formation constant* of [M(CN)44]2− is 7.70×10167.70×1016, where M is a generic metal. A 0.1400.140 mole quantity of M(NO3)2 is added to a liter of 0.9700.970 M NaCN solution. What is the concentration of M2+ ions at equilibrium? [M2+]=arrow_forward4. If I add the following will the system shifts forward, backward or remains the same? Ag, CrO, (s) = 2 Ag" (aq) + CrO,² (aq) d. Add Acid e. Add ammoniaarrow_forward6. A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 M acetic acid (CH3COOH) solution. (A) write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (B) Write the complete ionic equation for the reaction that occurs when few drops of sodium hydroxide solution are added to the buffer. Group of answer choices a.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq) (B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l) b.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq) (B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq) c.) (A) Na+ (aq)+ CH3COO-(aq)+ H+ (aq)+CI-(aq) --->CH3COOH(aq)+Na+(aq)+CI-(aq) (B) CH3COOH(aq) + OH-(aq)--->CH3COO-(aq)+H2O(l) d.) (A) CH3COO-(aq)+ H+ (aq) --->CH3COOH(aq) (B) CH3COOH(aq)+Na+(aq)+ OH-(aq)--->CH3COO-(aq)+H2O(l)+Na+(aq)arrow_forward
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