5. The following questions involve titrations of dimethylamine, (CH₂)2NH, a weak base, Kb = 2.2 x 104, with nitric acid, HNO3, a strong acid. A) Given the concentration of the acid and base are both 0.1M and 500 mL of dimethylamine is in the flask and nitric acid is in the burette, sketch the titration curve to a final volume of 1000 mL. Identify and label: the initial pH (+/-1) the final pH (+/-1) . . . . the equivalence point at an appropriate pH (+/- 1) and volume (+/- 100 mL) the buffer region at the appropriate pH (+/- 1) and volume (+/- 100 mL)

A 50.0 mL solution of Mg(OH)2 of unknown concentration is titrated with 0.348 M HCI. The equivalence point (end point) is reached after 62.8 mL of HCI were dispensed into the Mg(OH)2 solution. What is the molarity concentration of the base?

An aqueous solution of Ca(OH)2with a concentration of 0.188 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. How many moles of base were required to react completely with the acid in this reaction? How many moles of HCl were present in the original 25.00 mL of acid?

Fill in the missing words With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the form of Zn(OH)2 with the addition of 6.00 mL of NaOH, the number of moles of Zn2+ in this 10 mL brass stock solution is mmol. Therefore, there are mmol of Zn2+ in the entire 100-mL brass stock solution, which is g/mol). mg of Zn2+ (FW = 65

After 10.0 mL of a 0.020 M Ba(OH)2 (aq) are mixed with 15.0 mL of a 0.020 M KOH(aq), what is the molarity of [OH-]?

The flask contains 10.0 mL HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NaOH. It requires 11.0 mL of the NaOH solution to reach the end point of the titration.   What is the initial concentration of HCl?

6. Acid/base titration is a common method to determine the molarities of acids or bases, the molarity of certain salts can also be determined by titration. It took 22.34 mL of 0.5861 M HCl solution to neutralize 25.00 mL NaNO₂ solution. The acid- dissociation constant of HNO₂ is 4.511 × 10-¹. NaNO₂ + HCl → HNO₂ + NaCl Please answer the following questions. A What is pH of the NaNO₂ solution before titration? Hint, calculate the molarity of the NaNO₂ solution first. pH = Please provider your answer below. ( Check answer 7²² B. M HCl solution was added to the NaNO2 solution? pH = 00 0 Please provider your answer below. What is the pH when 12.78 mL of 0.5861 (0) Check answer C. What is the pH when 14.39 mL of 0.5861 M HCl solution was added to the NaNO₂ solution AFTER the equivalence point? pH = Please provider your answer below. 00 0 °C? pH= Please provider your answer below. Check answer What is the pH at equivalence point at 25 A → ← Check answer ← $ H $

what is the molarity of a solution of phosphoric acid (a tricrotic acid) if 10.00 mL of the phosphoric acid solution requires 38.11 mL of 0.2412 M NaOH solution to titrate it?

Suppose 0.473 grams of a solid monoprotic acid are titrated with 16.32 mL of 0.106 M NaOH.  What is the molar molar mass of the solid acid?

The principal ingredient of certain commercial antacids is calcium carbonate, CaCO3. A student titrates 25.0 mL of antacid with hydrochloric acid; the reaction is CaCO3 + 2HCl rightwards arrow CaCl2 + CO2 + H2O If 38.5 mL of 0.200 M HCl is required for complete reaction, what is the molarity of antacid? 0.254 M 0.154 M 0.015 M 0.025 M