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Calculate the pH value at the endpoint of titration of 0.1 M 100 mL oxalic acid, with 0.5 M 42.55 mL NaOH.
H2C2O4(aq) + 2 NaOH(aq) → Na2C2O4(aq) + 2 H2O(i)
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- The weak acid acetic acid, CH3COOH(aq), is titrated with strong base potassium hydroxide, KOH(aq). The pH at the equivalence point of the titration is determined by what species in solution? CH3COO− K+ KOH CH3COOH22+ CH3COOHZn(II) hydroxide is amphoteric (amphiprotic). Complete and balance the following equations. Include the phases of all species in the chemical equations. Complete and balance a chemical equation showing how an aqueous suspension of this compound reacts to the addition of a strong acid. Zn(OH)2(s)+2H+(aq) Complete and balance a chemical equation showing how an aqueous suspension of this compound reacts to the addition of a strong base. Zn(OH)2(s)+2OH−(aq)In a titration of acetic acid by sodium hydroxide, what is the pH of a 100.0 mL of a 0.1000 M CH3CHO2H(aq) solution after 25.00 mL of 0.2000 M NaOH(aq) has been added? The Ka of acetic acid is 1.75 x 10-5,
- A rainwater sample from Mondstadt was determined to contain 1.23 x 10⁻⁷ M of hyrdonium ion. Determine the pH and pOH of the rainwaterA solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of 0.0240M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.A 20.00 mL aliquot of sorbic acid solution (HC6H7O2) was titrated with 0.0985 M NaOH * (aq) using both an indicator and a pH meter. Ka (HC6H7O2) , is 1.7*10^ -5 . A total of 25.34 mL of 0.0985 M NaOH * (aq) was required to reach the equivalence point a) Calculate the molarity of the sorbic acid solution. b) Calculate the pH of the sorbic acid solution (use the RICE table) . c) .Calculate the pH and [C6H 7 O 2-] at the half-equivalence point . d) Calculate the pH at the equivalence point of the titration . (use Kb for hydrolysis of sorbate anion and RICE table ). e)Suggest an appropriate indicator for titration . Explain your choice . f) Calculate the pH of the solution after 10.00 mL of 0.0985 M NaOH * (aq) was added . (find moles of sorbic acid and sorbate and use Henderson Haselbalch equation ) Indicator pKa Phenolphthalein 9.3 Bromothymol blue 7.0 Methyl red. 5.0 Thymol blue. 2.0 Methyl violet…
- Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M nitric acid. The Kb for hydrazine is 3.00x10-6. H2NNH2(aq) +HNO3(aq) ⟶ [H2NNH3]+1(aq) + NO3-1(aq)What is the pH of the solution when 20.0 mL of 0.155 M of NH3(aq) is titrated with 15.0 mL of 0.225 M of HCl(aq)? The Kb of NH3 is 1.8 x 10-5.A solution is formed by adding 2.70 grams of solid sodium hypochlorite, NaClO, to 200.0 ml of 0.0210M calcium hypochlorite, Ca(ClO)₂. Calculate the pH of the resulting solution. You may assume that the sodium hypochlorite dissolve completely and that the change in volume is negligible with the addition of the solid.
- Calculate the pH of a mixture containing 0.23 M HONH2 and 0.44 M HONH3Cl. (Kb = 1.1 × 10–8) What is the pOH of the solution? pOH = _________A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedThe pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a) HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq). b) How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq)?