Determine the volume in mL of 0.251 M HBr(aq) needed to reach the equivalence (stoichiometric) point in the titration of 25.92 mL of 0.138 M (CH3)2NH(aq). The Kb of dimethylamine is 5.4 * 10^-4.

A pure organic compound has the formula C4H8SOx. A sample of a compound wasdecomposed; the sulfur was converted to sulfate and titrated in a modified version of theadsorption indicator procedure. From the following data, determine the correct formula forthe compound.Given: weight of sample = 12.64 mgBa(ClO4)2 needed for titration = 10.60 mL of 0.0100 M Ba(ClO4)2

A solution of malonic acid, H2C3H2O4H2C3H2O4 , was standardized by titration with 0.1000 M NaOHNaOH solution. If   21.68 mLmL  of the  NaOHNaOH solution were required to neutralize completely  13.00 mLmL  of the malonic acid solution, what is the molarity of the malonic acid solution?  H2C3H2O4+2NaOH→Na2C3H2O4+2H2OH2C3H2O4+2NaOH→Na2C3H2O4+2H2O

24.16 mL of 0.2704 M sodium hydroxide is titrated with 29.00 mL of phosphoric acid.  Calculate the molarity of phosphoric acid.

A chemistry graduate student is given 250. mL of a 1.50M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,=4.9 × 10 1º. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.84? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ?

Calculate the number of moles of F ions present in 6.0 mL of 0.00350M solution ZnF2(aq).

A student tries to determine experimentally the molar mass of aspirin (HAsp).She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is:HAsp(aq) + OH-(aq) ----> Asp-(aq) + H2O(l) What is the molar mass of aspirin?

2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

Consider the titration of 25.0 mL of 0.112 M acetic acid (CH, COOH, pK, = 4.75) with 0.131 M NaOH. CH;COOH(aq)+NaOH(aq) · CH, COO (aq) + H,O(1) + Na*(aq) Determine the initial pH of the 0.112 M acetic acid solution before NaOH is added. pH : Determine the pH of the solution after 10.0 mL of 0.131 M NaOH is added. pH =

A fruit juice contains an unknown percentage of citric acid. During a titration 33.50 cm³ of 0.0102 M sodium hydroxide is required to neutralise the citric acid in 50.0 cm³ of fruit juice. The unbalanced reaction equation is given in Figure 10. Citric acid is a triprotic acid – it can donate three H⁺ ions in aqueous solution. You can assume that the density of the fruit juice is the same as that of water. What is the percentage of citric acid in the sample? [Round the answer to three decimals. Do not type in the percentage sign. Use a decimal point.]