Question

In: Chemistry

You add 0.535 g of NaOH to 100.0 mL of water at 25

Expert Solution

Molar mass of NaOH = atomic mass of Na + atomic mass of O + atomic mass of H

= 23 + 16 + 1

= 40 gmol ^-1

Given mass of NaOH , M = 0.535 g

So no.of moles ,

Molarity of the solution ,

M = 0.134 M

NaOH Na⁺ + OH ^-

1 mole of NaOH produces 1 mole of OH^-

So concentration of [OH^-] = concentration of NaOH

= 0.134 M

pOH = - log[OH^-]

= - log 0.134

= 0.87

pH = 14-pOH

= 14-0.87

= 13.13

pH = -log[H₃O⁺]

[H₃O⁺]= 10^-pH

= 10 ^-13.13

= 7.4810^-14 M

queen_honey_blossom answered 2 hours ago

You add 7.50 mL of 0.050 M NaOH to 50.00 mL of pure water, and to...

You add 7.50 mL of 0.050 M NaOH to 50.00 mL of pure water, and to this mixture you then add 1.50 mL of 0.200 HCl. What will be the pH of the resulting solution? 2.11 11.10 11.89 7.00 2.49

A 25 g piece of metal is dropped into 100.0 g sample of water. The water...

A 25 g piece of metal is dropped into 100.0 g sample of water. The water temperature drops by 5.0 C. The piece of metal's temperature increases by 85 C. What is the specific heat of this piece of metal? (The specific heat of water is 4.18 J/gC)

If you combine 360.0 mL of water at 25.00 °C and 100.0 mL of water at...

If you combine 360.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

If you combine 330.0 mL of water at 25.00 °C and 100.0 mL of water at...

If you combine 330.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

1.250 g of H2C2O4 are dissolved into 100.0 ml of water which is then titrated with...

1.250 g of H2C2O4 are dissolved into 100.0 ml of water which is then titrated with 28.56 ml of NaOH solution. What is the molarity of the NaOH solution? H2C2O4 + NaOH arrow Na2C2O4 + H2O (not balanced) Select one: a. 0.6942 M b. 2.957 M c. 0.4862 M d. 1.945 M e. The correct answer is not given as an option.

A. You have 100.0 mL of 0.050 M acetic acid in water at 25 C. What...

A. You have 100.0 mL of 0.050 M acetic acid in water at 25 C. What are thre pH and pOH of this solution. B.What is the pKa for acetic acid? C.The pKa of trifluoroacetic acid (CF3CO2H) is 0.23. Which is a stronger acid? that or acetic acid?

You dissolve 0.735 g of salt cyclphexylamine chloride with enough water in a 100.0 ml volumetric...

You dissolve 0.735 g of salt cyclphexylamine chloride with enough water in a 100.0 ml volumetric flask. You then titrate the solution with 0.050 M sodium hydroxide. Ka of cyclohexylamine is 2.71E-11. a) calculate NaOH volume needed of reach the equivalent point. b) calculate the pH at the equivalent point.

f you combine 320.0 mL of water at 25.00 °C and 100.0 mL of water at...

f you combine 320.0 mL of water at 25.00 °C and 100.0 mL of water at 95.00 °C, what is the final temperature of the mixture? Use 1.00 g/mL as the density of water.

131 g of metal at 100.0 oC is added to 60.0 mL of water at 26.0...

131 g of metal at 100.0 oC is added to 60.0 mL of water at 26.0 oC. The equilibrium temperature reaches 39.9 oC. The specific heat of water is 4.184 J/g.K. Assuming the heat capacity of the calorimeter is negligible, calculate the specific heat of the metal.

A 1.00-g sample of piperazine hexahydrate is dissolved in enough water to produce 100.0 mL of...

A 1.00-g sample of piperazine hexahydrate is dissolved in enough water to produce 100.0 mL of solution and is titrated with 0.500 M HCl. A.) What is the initial pH of the solution, before any titrant is added? B.) The percent neutralization points for a titration indicate the percent of the reagent that has reacted. For example, at the 25% neutralization point for piperazine, 75% (0.75×[Pip]) of the base remains, and 25% is neutralized to form PipH+. Calculate the pH...