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- 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-equivalencWhat do you call the stage of the titration in which the number of moles of the titrant is the same stoichiometrically as the number of moles of the analyte? end stage post-equivalence equivalence pre-equivalence4. Are ‘equivalence point’ and ‘end point’ the same? If yes, why? Otherwise, differentiate the two. 5. Aside from repeating the experiment, what can be done to remedy a sample that is ‘over-titrated’.
- The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?What is the solubility of calcite (CaCO3) in grams per milliliter at a temperature at which its Ksp is 9.93×10-9?A student titrates a 50.00mL sample of water with 17.85mL of 0.0100M ethylenediaminetetraacetic acid at pH = 10 to the Erio T indicator end point. What is the hardness of the water sample in ppm CaCO3 (Molar mass = 100.1 g/mol)?
- A mixture of NaOH (M.wt = 40) and Na2CO3 (M.wt = 106) is titrated with 0.3 M HCl, requiring 30 mL for phenolphthalein end point and an additional 15 mL to reach the modified methyl orange end point, How many milligrams of NaOH and Na2CO3 are in the mixture *What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of 4.00? Report to 3 sig figsA 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091 M NaOH, requiring 29.5 mL to reach the end point. Determine the compound’s equivalent weight.
- 1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…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)Carly the chemist consistently obtained a dark pink endpoint in all of her titrations in her KHP determination lab. What type of errorr is this and how would it affec tthe accuracy and precision of her results?