Solubility of Ca(OH)2a) Give a balanced reaction equation for the reaction of Ca(OH)2 with hydrochloric acid.b) Describe what happens when you add a sodium hydroxide solution to the solution above(5a). What is the reaction product?
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a) Give a balanced reaction equation for the reaction of Ca(OH)2 with hydrochloric acid.
b) Describe what happens when you add a sodium hydroxide solution to the solution above
(5a). What is the reaction product?
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- What products should form during the reaction between hydrochloric acid, HCl(aq), and a solution of calcium hydroxide, Ca(OH)2(aq)? Write a balanced chemical equation for the reaction.Write the balanced neutralization reaction between Ca(OH)₂ and HBr.The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.
- 12) What is the concentration of H+ ions in HCl whose pH is 6.9?KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP– . HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a) Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b) Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c) Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g mol and at 25 °C has a pKa of 5.4.The active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.
- Iron in drinking water is removed by precipitation of the Fe3+ ion by reaction with NaOH to produce iron(III) hydroxide. Write the balanced chemical equation and the net ionic equation for this reaction.A 50.0 mL solution of Ca(OH) 2 with an unknown concentration was titrated with 0.340 M HNO3. To reach the endpoint, a total of 26.2 mL of HNO3 was required. Given that 0.00891 mol of HNO3 are used in the titration, What quantity in moles of Ca(OH)2 had to be present in the initial reaction?5. Hydrogen cyanide has the chemical formula HCN. The compound occurs as a colourless gas or a pale blue liquid. Its solution in water is called hydrocyanic acid. It reacts with water as per the reaction. What is the pH of a 0.30 mol/L solution of the above acid (K=6.2 x 10- 10)? HCN(aq) + HO({) ↔ CN-(aq) + HO+(aq) 2 3
- 8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca1OH22?4. Suppose you had a sample of Hydrobromic acid that had a molarity of 0.1 and you had 42 ml of it. If you added 20 ml of 0.15 M NaOH, what is the pH of the resulting solution? NaOH + HBr -> NaBr H2O
