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What is the pH of a 0.173 M solution of a hydrogen sulfide? The pKa at the temperature of the experiment is equal to 7.03.
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- There are many organic acids and bases in our cells, and their presence modifies the pH of the fluids inside them. It is useful to be able to assess the pH of solutions of acids and bases and to make inferences from measured values of the pH. A solution of equal concentrations of lactic acid and sodium lactate was found to have pH= 3.08. (a) What are the values of pKa and Ka of lactic acid? (b) What would the pH be if the acid had twice the concentration of the salt?a) Calculate the pH of an aqueous solution of the salt NaA, which was made to a concentration of 0.080 M NaA. The Ka of the weak acid HA is 2.0 x 10-5. Your pH should go to two places past the decimal point (i.e. 1.35). b) Aniline, C6H5NH2, has a pKb of 9.40. What is the pH of a solution which is 0.12 M in aniline and 0.38 M in anilinium ion, C6H5NH3+? Your answer should be to two places past the decimal.The pKa of a particular weak acid is 4.85. What is the pH of the weak acid solution when exactly half of the acid is neutralized?
- Calculate the pH for a mixture of one mole of benzoic acid and one mole of sodium benzoate. The pKa of benzoic acid is 4.2. 0 2 8 8 2 8 2 5 6The ionization constant Ka for nitrous acid is 4.6x10⁻⁴. What are the the pKa for nitrous acid and the pH of a 0.1 M solution of this weak acid?4a) Write an equation for the neutralization reaction of sodium acetate in solution upon addition of HCl.
- Consider a biochemical reaction that is taking place in a 0.1 M buffer. The initial pH is 7.4, and the pKa of the buffer is 7.2. If, in a final reaction volume of 1.0 mL, 10 micromol of protons are generated, what would be the final pH of the solution?ACID-BASE EQUILIBRIA AND SALT EQUILIBRIA (COMMON-ION EFFECT, BUFFER AND SOLUBILITY EQUILIBRIA) The pH of the given solution of lactic acid and lactate is 5.24. Calculate the pKa of lactic acid, when the concentration of lactic acid and lactate are 0.024 M and 0.087 M respectively.Given the identity of the base, its concentration and pKb, determine the pH of a solution of the base. Show all work A student dissolves 0.750 moles ofNaA (where A is the anion/conjugate base of a generic weak monoprotic acid, HA) in 1 liter of water. What is the resulting pH of the solution if the generic acid (HA) has a pka of 3.26?
- Given that pH + pOH = 14 and that the concentration of water in a solution of water is 55.5 M, show that the pKa of water is 15.7.Discuss and give a reason for the pollution problem associated with acid rain?Phosphorus can be prepared from calcium phosphate by the following reaction: 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) ➜ 6CaSiO3(s) + P4(s) + 10CO(g) Phosphorite is a mineral that contains Ca3(PO4)2 (molar mass: 310.174 g/mol) along with other non-phosphorus-containing compounds. The phosphorite used is 68.5% Ca3(PO4)2 by mass. A. What amount of phosphorite is needed to completely react with 2.00 kg SiO2 (molar mass: 60.083 g/mol)? B. How much of an initial 2.65-kg SiO2 remains unreacted if 0.750 kg of phosphorite was used up to produce phosphorus? C. What is the maximum amount of P4 (molar mass: 123.896 g/mol) that can be obtained from 5.00 kg of phosphorite? D. If the percent yield of this process is 73.5%, how much phosphorus is collected from 5.00 kg of phosphorite?