A volume of 500.0 mL of 0.130 M NaOHNaOH is added to 565 mL of 0.200 M weak acid (?a=6.13×10−5). What is the pHpH of the resulting buffer? HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)
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A volume of 500.0 mL of 0.130 M NaOHNaOH is added to 565 mL of 0.200 M weak acid (?a=6.13×10−5). What is the pHpH of the resulting buffer?
HA(aq)+OH−(aq)⟶H2O(l)+A−(aq)
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- you are given 1.8 M acetic acid solution (CH3COOH) and solid sodium acetate trihydrate (NaOOCCH3 X 3 H2O) the two buffer solutions are identical. if 5.00 mL of a 1.0 M NaOH solution is added to one of the buffers what would be the resulting pH after addition?Consider an analyte solution of 50.0 mL of 0.050 M hydrochloric acid, HCl, titrated against 0.10 M sodium hydroxide, NaOH (g) After adding 37.50 mL of the NaOH, 50% past the equivalence point, what ions or molecules are present in the solution? (h) Which of the species you identified in part (g) will determine the pH of the solution?Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid with a concentration of 0.50 M is titrated using standardized 0.25 M NaOH. C6H5COOH(s) ⇄ C6H5COO–(aq) + H+(aq) Ka = 6.46 x 10–5 a.Calculate the pH of the solution after the following amounts of NaOH have been added… 0 mL 10 mL 85 mL b. State whether the solution at the equivalence point of the titration is acidic, basic, or neutral. Explain your reasoning. c. How many mL of 0.25 M NaOH need to be added in order to make the ideal buffer solution?
- In a titration experiment, 0.27 M NaOH is added to 21.8 mL of a 0.35 M H3PO4 solution and reacts according to the equation: 3 NaOH (aq) + H3PO4 (aq)--------------> Na3PO4 (aq) + 3 H2O (aq) How many milliliters of sodium hydroxide solution have been added at the equivalence point (end point)?A student performs a titration between 10.0 mL of a 0.25 M weak acid HA(aq) (Ka = 2.45 x 10 −5) and 0.25 M sodium hydroxide, NaOH(aq). Which of the following is true for the titration when 5.0 mL of sodium hydroxide has been added? HA(aq) + NaOH(aq) → NaA(aq) + H2O(l) The pH of the solution will be equal to −log(Ka). A buffer has formed between the sodium hydroxide and the conjugate acid of sodium hydroxide. Exactly half of the sodium hydroxide has reacted and Kb is equal to Ka. The titration is at equivalence.In a titration experiment, 0.84 M KOH is added to 34.6 mL of a 0.67 M H2SO4 solution and reacts according to the equation: 2 KOH (aq) + H2SO4 (aq)--------------> K2SO4 (aq) + 2 H2O (aq) How many milliliters of potassium hydroxide solution have been added at the equivalence point (end point)? 2. In a titration experiment, 0.27 M NaOH is added to 21.8 mL of a 0.35 M H3PO4 solution and reacts according to the equation: 3 NaOH (aq) + H3PO4 (aq)--------------> Na3PO4 (aq) + 3 H2O (aq) How many milliliters of sodium hydroxide solution have been added at the equivalence point (end point)?
- Consider the following acid base titration between H2C3H5O3 (aq) with KOH (aq). A)Write a complete balanced equation. B) If 25.0 mL of the acid required 13.6 mL of 0.0789 M of the base to reach the equivalence point, what is the concentration of the acid? C)Which of the reactant is the limiting reactant?The endpoint in a titration was reached when 23.5 mL of a 0.0100 M solution of NaOH was added to 0.0200 L of an HCl solution of unknown concentration. The neutralization reaction is as follows: HCl (aq) + NaOH (aq) → NaCl (aq) + H₂O(l) Calculate the Molarity of the HCl solution.A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.615 M NaOH. The equivalence point is reached when 33.6 mL are added. What is the unknown acid?
- A solution of tartaric acid (H2C4H6O6) with a known concentration of 0.155 M H2C4H4O6 is titrated with a 0.425 M NaOH solution. How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H2C4H4O6, according to the following balanced chemical equation : H2C4H4O6 + 2 NaOH --> Na2C4H4O6 + 2H2OA 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask. After the addition of methyl orange, a titration with 0.0045 M HCl was performed. The endpoint was reached after 8.72 mL of the acid was added. What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction? What is the molar concentration of hydroxide in the saturated solution? What is the molar concentration of Magnesium ion in solution?You perform an acid-base titration to standardize an HCl solution by placing 50.00 mL of HCl in a flask with a few drops of indicator solution. You put 0.1524 M NaOH into the buret, and the initial reading is 0.55 mL. At the end point, the buret read-ing is 33.87 mL. What is the concentration of the HCl solution?