Question Potassium hydroxide is very soluble in water, resulting in extremely basic solutions. A 121 g...
Potassium hydroxide is very soluble in water, resulting in extremely basic solutions. A 121 g sample KOH is dissolved in water at 25 °C to make up 100.0 mL of solution. The molar mass of KOH is 56.11 3. What is the pH of the solution at 25.0°C? • Round the answer to two decimal places.
14 grams of impure koh ( potassium hydroxide ) was dissolved in water to make 100 ml of solution. the solution was then titrated with 1.26 m nitric acid solution. 40.0 ml of the acid required 25.0 ml of alkali solution. determine the percentage koh of the sample
Sodium hydroxide is extremely soluble in water. At a certain temperature, a saturated solution contains 567 g NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution. concentration: If 8.67 g of CuNO, is dissolved in water to make a 0.250 M solution, what is the volume of the solution in milliliters? volume: mL
When a 7.82-g sample of solid potassium hydroxide dissolves in 100.0 g of water in a coffee-cup calorimeter, the temperature rises from 22.7 °C to 59.2 °C. What is ΔH for the dissolution of KOH in water, as shown below? KOH(s) → K+(aq) + OH−(aq) Assume that all solutions have the same specific heat as water.
A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid-base indicator is added and the resulting solution is titrated with 2.50 M HCl(aq)solution. The indicator changes color signaling that the equivalence point has been reached after 17.0 mL of the hydrochloric acid solution has been added. Part B What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+? Li+ Na+ K+ Rb+ Cs+ Part A What is...
Could someone answer the following questions? 1) 11.2 g of potassium hydroxide (KOH) is dissolved in sufficient water to make 1 L of solution. What is the concentration of KOH in the solution? a. 0.02 mol/L b. 0.1 mol/L c. 0.2 mol/L d. 0.01 mol/L 2) If the solution is neutral, which of the following must be true? a. [OH-] = [H2O] b. [H+] > [OH-] c. [H+] < [OH-] d. [H+] = [OH-] 3)A student titrates 0.5222 grams of...
A 4.75-g sample of an unknown compound is dissolved in enough water to make 100.0 mL of solution. This solution has an osmotic pressure of 25.0 torr at 25oC. Find the molar mass of the unknown.
A 5.00 g quantity of a diprotic acid (H2A) was dissolved in water and made up to exactly 250 mL. Calculate the molar mass (in g/mol) of the acid if 25.0 mL of this solution reuired 11.1 mL of 1.00 M KOH for neutralization.
A 4.36 g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid-base indicator is added, and the resulting solution is titrated with 2.50 M solution of HCl. The indicator changes colour, signalling that the equivalence point has been reached after 17.0 mL of the hydrochloric acid solution has been added. Determine the molality of this alkali metal hydroxide solution and What is the mass percentage of the metal hydroxide in the solution? Determine...
A 6.25−g quantity of a diprotic acid was dissolved in water and made up to exactly 275 mL. Calculate the molar mass of the acid if 25.0 mL of this solution required 10.8 mL of 1.00 M KOH for neutralization. Assume that both protons of the acid were titrated.