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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_forward3. Sulphuric acid (H2SO4 ), used in the manufacture of fertilizers, undergo decomposition and the acid dissociation constants are given as: Ka1 = 1x 10° and K.2 = 1.2 x 10¬2 . The initial concentration of sulphuric acid is given as 0.040M. (i) Write the dissociation reactions. (ii) Calculate the concentration of [HS0, ] and [SO]. (iii) Calculate the pH of the acid solution. (iv) Write a discussion on the behaviour of polyprotic acids. (50 -100 words) Given: lon product constant for water, K, = 1 x 10-14arrow_forwardCopper(I) ions in aqueous solution react with NH3(aq) according toCu+(aq) + 2NH3(aq) → Cu(NH3)2+(aq) Kf = 6.3 × 1010Calculate the solubility (in g·L-1) of CuBr(s) (Ksp = 6.3 × 10-9) in 0.62 M NH3(aq).62.3solubility of CuBr(s):arrow_forward
- Consider the reaction: HCI(aq) + NH, (ag) – NH,Cl(aq) Where 20.00 mL of 0.100 M NH, (aq) is added to 10.00 mL of 0.200 M HCl(aq). Order the solution components (excluding water) from highest to lowest concentration. O [OH¯] > [NH3] > [Na*] > [Cl¯] > [H,O*] O (CI ] = [NH†] > [NH,] = [H,O*]> [OH¯] O [H,0*)> [Cl¯] > [NH,] > [NH†]> [OH) O [NH]= [OH"] > [H,O*] = [CI¯] > [NH,] O [H,0*] = [CI¯] > [NH,] > [NH ] = [OH] O [NH,CI] = [NH,] = [HCl] O [CI] > [NH†]> [H,O+] > [NH,] > [OH ] O INH,CI] > [NH3] > [HCl] O None of thesearrow_forwardThe solubility of TICI (thallium(I) chloride), an intermediate formed when thallium is being isolated from ores, is 3.12 grams per liter at 20 °C. What is its solubility product?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_forward
- Aluminum 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_forwardThe 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_forward
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