in a titration, if the mass of KHP in three experimental solutions are 0.467,0.48, and 0.48 and the volume of NaOH IN THE exp are 22,29,24 respectively in order to the masses of KHP.find the molarity of NaOH of each experiment. calculate the avarage molarity of NaOH M.

2. In the second titration, the molar mass of an unknown monoprotic acid is calculated.  If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question Which is 0.1186

GW 18b 1. A 20.0 mL sample of a 0.240 M hydrofluoric acid (HF) solution is titrated with 0.200 M NaOH. Determine: (a) pH of the acid solution before any base is added; (b) volume (in mL) of base needed to get to the equivalence point; (c) pH halfway to equivalence point; (d) pH at equivalence point; (e) pH when 0.100 mL NaOH is added beyond the equivalence point. (K₂ of HF = 7.1 × 104)

In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a)  Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b)  Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c)  Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.

4. What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH,CH;COOH with 0.100 M NaOH? a) before the addition of any NaOH; b) after the addition of 10.00 mL of 0.100 M NaOH; c) after the addition of 12.50 mL of 0.100 M NaOH; d) after the addition of 25.00 mL of 0.100 M NaOH; e) after the addition of 26.00 mL of 0.100 M NaOH.

After the benzoate ion is separated from methyl benzoate because of their differences in solubility, what happens when HCI is added to the benzoate ion dissolved in water? OHCI donates a proton to the benzoate ion, resulting in benzoic acid, which is not soluble in water HCI accepts a proton from the benzoate ion, resulting in benzoic acid, which is not soluble in water HCI donates a proton to the benzoate ion, resulting in benzoic acid, which is soluble in water OHCI accepts a proton from the benzoate ion, resulting in benzoic acid, which is soluble in water

Calculate the pH for each of the cases in the titration of 35.0 mL of 0.240 M KOH(aq) with 0.240 M HCl(aq). Note: Enter your answers with two decimal places. before addition of any HCl: after addition of 13.5 mL HCl: after addition of 21.5 mL HCl: after addition of 35.0 mL HCl: after addition of 41.5 mL HCl: after addition of 50.0 mL HCl:

Write the titration reaction of 100 mL of 0.100 M anilinium bromide (“aminobenzene . HBr”) +.100 M NaOH.

A student performs the titration of 88.0 mL of 1.1 M HCI (in flask) with 13.0 mL of 0.20 M NaOH (in burette). What is the pH at this point in the titration? (Hint: Use a barf table.) Your Answer: Answer

5. You use a 0.1380 M HCI to standardize an NaOH solution. The burets below show initial and final volume readings for the titration to the perfect endpoint. Calculate the appropriate volume ratio (Va/Vb or Vb/Va ratio) and the [NaOH]. Acid Buret Reading (mL) initial final cumpasın INHI IN ||| Base Buret Reading (mL) initial final ייייייי |||||