If the system CaCO3(s) + 2H+(aq) --> Ca2+(aq) + CO2(g) + H2O(l) is saturated with respect to CaCO3, what will happen to the Ca2+ if the pH of the solution begins to decrease? Explain your answer.
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- 5. What concentration of acetate ion (CH3CO2') in 0.500 M CH3CO2H produces a buffer solution with pH = 5.00? (Ka = 1.8 x 10-5) CH;CO2H (aq) H20 (I) CH;CO, (aq) H30* (aq) + 6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH;CO2H) to 1.00LH,0. What is the pH of the solution at equilibrium? (K, 1.8 x 10°)Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2 (s). (a) If solid CaCl2 is added to this solution, will the amount of solid CaF2 at the bottom of the beaker increase, decrease or remain the same? (b) Will the concentration of Ca2+ ions in solution increase or decrease?In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…
- A buffer solution is prepared from a generic weak acid "HG" and the salt KG. The K, for HG is 3.7 x 10. What is the correct equation for the dominant equilibrium in the buffer solution? O KG + HG HKG' + G O KG + H,O KOH- + HG O HG + H,O OH- + H2G O HG + H,O G + H2O* G+ H20 OH + HGThe thermodynamic solubility product of AGCN is 6.0x10-17. (a) What is [Ag+] in a 0.033 M KNO3 solution? 4.0 7.7e-9 X mol·L-1 (b) What is [Ag+] in a 0.033 M KCN solution? 4.0 1.8e-15 X mol·L-1One can calculate the molar solubility of a conic marble sample, predominantly made of CACO3, when exposed to acid rain with a pH of 4.34 using the following information: CaCO3(6) + H2O1) + CO2(aq) Ca2+, (aq) + 2 НСОЗ (аq) K = ? CaCO3(6) = Ca"(aq) + CO3“ (aq) Ksp = 2.8 x 109 CO2{aq) + 2 H2O) = H3O*(aq) + HCO3 (aq) K1 = 4.4 x 10-7 HCO3 (aq) + H2O) = H30*(aq) + CO3 (aq) K2 = 4.7 x 1011 2 H2O1) = H30* (aq) + OH (aq) Kw = 1.0 x 10-14 A water sample from around the marble is collected into a conical container. Assuming that the calcium is purely from the marble sample, and basing your calculations off of the molar solubility, calculate how many grams of calcium are present in this water sample. Note that the cone has a base radius of 10.00mm and a height of 480.8mm. molar solubility of CaCO3 = M amount of calcium x 10-3 g %3D
- One drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0 cm3 of a phosphate buffer that is 0.040 mol dm-3 in KH2PO4(aq) and 0.020 mol dm-3 in K2HPO4(aq). Calculate the resulting pH of the solution given that the second acid dissociation constant, pKa2, for phosphoric acid is 7.21.Consider the titration of a 50.00 mL sample of 0.100 M ethylamine, C2H5NH2, with 0.100 M HCl (aq., 25 oC). The Kb C2H5NH2 = 6.41 x 10–4. What is the pH after 25.00 mL of HCl has been added?To a buffer containing 0.150 mol NH3 and 0.250 mol NH4 0.050 mol of HCl (aq) is added. Calculate the pH of the solution given that Ko of NH3 is 1.8 x 10-5.
- Consider a flask containing 25.00 mL of 0.100M sodium benzoate (NaC, H5C00). This is titrated with a 0.110 M nitric acid solution from a burette. Given: K, of C,H;co0" is 1.6 x 10-10. Determine the pH of the solution in the flask after 32.00 mL of the acid has been added? You must show any reaction equation(s) that you may think are necessary. Determine the pH of the solution in the flask at the half-way point of the titration.Calculate the Molar Solubility at 25.0 oC of an aqueous solution of calcium phosphate, Ca3(PO4)2, given that its Ksp = 1.20 x 10–26 at 25.0 oC.Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)