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- The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)For Ca2+ and Mg2+ determinations in a tap water sample, two 50 mL aliquots were pipetted and placed in different Erlenmeyer flasks. The first of them had the pH adjusted to 12 (Ca2+ titration) and the second to 10 (Ca2+ +Mg2+ titration). The volumes of EDTA (5.07*10-3 mol/L) used in the first and second titrations were 2.40 and 4.80 mL, respectively. Calculate: a) The concentration of Ca2+ in mg/L in the water sampleb) The concentration of Mg2+ in mg/L in the water sample
- A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)A 10.00cm3 portion of the 100.00cm3 HCl solut was taken from the volumetric flask and was titrated with KOH (aq). It was neeutralized by 24.35cm3 of potassium hydroxide od concentration 0.0500moldm-3. Calculate the concentrat of the original concentrated hydrochloric acid in moldm-3.Consider the titration of 25 mL of 0.1 M HCHO2 (known as formic acid and has a Ka of 1.8 x 10-4) with 0.1 M of the strong base KOH. Clearly calculate the initial pH, the pH at half way to the equivalence point, the pH at the equivalence point, and the pH after the addition of infinite excess KOH.
- If 21.6 mL of 0.107 M acid with a pKa of 5.16 is titrated with 0.105 M NaOH solution, what is the pH of the titration mixture at halfway to the equivalence point?acetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an erlenmeyer, you titrate 50 mL of this acid with 0.103 M NaOH and the phenolphtalein indicator duplo. The volume of NaOH needed to reach the equivalence point in both experiments was 48.96 mL and 49.11 mL. a. Write down the equilibrium reaction of dissolving vinegar in water, then write down the equation that reflects the acidic equilibrium constant!b. Calculate the average volume of NaOH needed to reach the equivalence point!c. Calculate the acidity of the vinegar in this sample!d. Calculate the initial pH of the vinegar solution before titrating!e. Calculate the pH at the equivalence point80.00 mL of 0.1000 M NaOH was be needed to reach the equivalence point in a titration with 25.00 mL of a triprotic acid. What is the concentration of the triprotic acid solution? Show your full calculation using 1-2 line unit analysis.
- What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalencGenerate a titration curve for 25.0 mL of 0.7233 M H3PO4, with 1.256 M NaOH as the titrant, given the following total volumes of titrant dispensed. H3PO4 ⇌ H2PO4- Ka1 = 7.11 x 10 -3 H2PO4- ⇌ HPO4 -2 Ka2 = 6.32 x 10 -8 HPO4 -2 ⇌ PO4 -3 Ka3 = 4.50 x 10 -13 V NaOH (mL): 0.00, 2.0, 12.0, 20.0, 30.0, 38.0, 45.0, 57.0, 66.0, 70.0, 85.01.Why is more than one accurate titration carried out? 2.Explain why hydrochloric acid is not used as a primary standard. 3.Can any of the following be used as primary standards: NaOH, H2SO4, HNO3? Explain your answer.