The barium oxide is a strong electrolye:  BaO(s) + H2O(l) → Ba2+(aq) + 2 OH−(aq). What is the pH of a solution prepared by dissolving 0.175 g of solid BaO in enough water to make 1.00 L of aqueous solution

A chemistry graduate student is given 125. mL of a 0.80M ammonia (NH3) solution. Ammonia is a weak base with K₂ = 1.8 × 10. What mass of NHÂBr should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.55? 4 You may assume that the volume of the solution doesn't change when the NH Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 × S

What is the pH of a 0.10 M N(CH3)3(aq)? The base ionization constant  of trimethylamine is Kb= 6.5×10–5. Enter your answer with correct units and significant figures.

The Kw of water at 100°C is 5.62 x 10-13. What is the pH of water at this temperature?

ion The following table shows data from the titration of four 25.0 mL samples of a perchloric acid solution, HCIO4(aq), using a 0.225 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 25.0 mL of HCIO4 with 0.225 mol/L NaOH(aq) final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint Trial 1 Use the data in the table below to answer the next two questions. Trial 2 Trial 3 Trial 4 Trial mL . . . mL mL 1 mL 19.9 0.4 2 Using the chart above, provide the volume of NaOH added for each of the trials. 38.8 3 19.3 19.9 0.2 4 38.4 19.3 blue green green green DELL

The acidity of a solution is measured by its pH. If Ht represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH - log Ht| Based on careful measurements and calculations, a chemist examines two solutions and asserts: "The hydrogen ion concentration of Solution A is 65.86% greater than the hydrogen ion concentration of Solution B." If the pH of solution B is 10.00, determine the pH of Solution A. Report your answer to two decimal places. Solution A has pH equal to Number (Report to the nearest 0.01)

The acid dissociation constant K of boric acid (H₂BO3) is 5.8 × 10-¹0. Calculate the pH of a 5.6M solution of boric acid. Round your answer to 1 decimal place. pH = 0 X 6

Chemistry The label of an energy drink states that it contains approximately 80 mg of caffeine (C8H10N4O2) per 250 mL serving. If the caffeine is a weak base with a basicity constant of 2.5 × × 10-4, what is the pH of the drink? (Only caffeine is considered to contribute to the pH of the drink.)

Determine the pH of a 1.497 M solution of potassium cyanide (KCN) in water. Ka for HCN is 6.17 × 10–10. Enter your response in pH units to the nearest 0.01.

Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH3(aq) + HCl(aq) – ->