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- What is the pH of a solution that results from mixing together equal volumes of a 0.150 M solution of acetic acid and a 0.075 M solution of sodium hydroxide? (pKa of acetic acid = 4.75) Express the answer to two decimal places.Determine the pka of an acid whose concentration is 0.100M and pH is 2.86.We mix 0.08 moles of chloroacetic acid (ClCH2COOH) and 0.04 moles of sodium chloroacetate (ClCH2COONa) in 1.0 L of water (pKa = 2,865). Find the pH of a solution prepared by dissolving the following compounds in a final volume of 1L: 0.08 moles of ClCH2COOH, 0.04 moles of ClCH2COONa, 0.05 moles of HNO3 and 0.06 moles of NaOH
- What is the Ka or Kb expression for NH4Cl and Na2CO3? What is the value of Ka or Kb for both chemicals? I got a pH of 6.77 for 0.1 M NH4Cl and a pH of 11.21 for 0.1 M Na2CO3.What is the reason for finding the 1/2 equivalence point? Select one: a. To determine the moles of acid present b. To find the pH of the base c. To find the pKa of the acid d. To determine the moles of base consumed e. To find the pH of the acidpH calculation after the second equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 69.4 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5
- 1. The ionization constant (Kb) of trimethylamine ((CH)3)3N) is 7.40 x 10–5. If 5.911 grams of trimethylamine is dissolved in 50.0 mL of water, what are the equilibrium concentration of all species present? 2. A buildup of a certain monoprotic acid in the muscle tissues can cause pain during extreme physical activities. A 0.0288 M solution of this acid is found to have a pH of 2.345. Based on the table below, what most likely is the identity of this unknown acid?A 1.0 M solution of a compound with 2 ionizable groups (pKa’s = 6.2 and 9.5; 100 mL total) has a pH of 6.8. If a biochemist adds 60 mL of 1.0 M HCl to this solution, the solution will change to pH: A) 5.60 B) 8.90 C) 9.13 D) 9.32 E) The pH cannot be determined from this information. I believe the answer is A, but I am saying this based on a guess: adding acid will lower the value of 6.8, and out of all the answers only 5.60 is lower than 6.8. But what are the maths and chemistry behind this? I'm not sure. Thank you for your help.Aqueous acids may be placed in order of acid strength according to their pka values. In the following, the stronger acids are nearer the top. HClO4(aq) ➡ H+(aq) + ClO-4(aq) HCl(aq) ➡ H+(aq) + Cl-aq) CH3CO2H(aq) ➡ CH3CO2-(aq) + H+(aq) H2O(l) ➡ H+(aq) + OH-(aq). Give one piece of experimental evidence to justify the above order. Define ka and pka
- pH calculation after the first equivalence point: Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5A solution is made by dissolving 44.1 g of Ba(NO₂)₂ in 500.0 mL of water. (a) Does Ba²⁺ have any acidic or basic properties? (b) Does NO₂⁻ have any acidic or basic properties? (c) As NO₂⁻ is a base, write the basic equilibrium equation that exists in solution (d) What is the value of Kb for NO₂⁻? The Ka of HNO₂ is 4.5 × 10⁻⁴. (e) Determine the pH of the solutionWhich of the following statements is true? A. A weak acid solution can be diluted with enough water to produce a solution with a pH greater than 7.00 at 25°C. B. Diluting a weak acid solution by a factor of ten will always decrease its pKa by 1. C. A weak base solution will always have a lower concentration of OH‒ than a strong base solution. D. A weak base solution will always have a pH of 7.00 or greater at 25°C. D. Correct Why is C false and not true??