1) A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....

1) A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH after 600.0 mL of the acid has been added.

2) A 100.0-mL sample of 0.100 M HCHO₂ is titrated with 0.200 M NaOH. Calculate the pH after adding 30.00 mL of the base.

Expert Solution

queen_honey_blossom answered 2 years ago

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid....

1. A 100.0-mL sample of 0.500 M sodium hydroxide is titrated with 0.100 M nitric acid. Calculate the pH after 400.0 mL of acid has been added. 2. A 1.0-L buffer solution contains 0.100 mol HCN and 0.100 mol LiCN. The value of Ka for HCN is 4.9 x 10-10. Because the initial amounts of acid and conjugate base are equal, the pH of the buffer is equal to pKa = -log (4.9 x 10-10) = 9.31. Calculate the new...

Part A A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric...

Part A A 50.0-mL sample of 0.200 M sodium hydroxide is titrated with 0.200 M nitric acid. Calculate the pH of the solution, after you add a total of 51.9 mL 0.200 M HNO3. Express your answer using two decimal places. Part B A 39.0 mL sample of 0.146 M HNO2 is titrated with 0.300 M KOH. (Ka for HNO2 is 4.57×10−4.) Determine the pH at the equivalence point for the titration of HNO2 and KOH .

For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide,...

For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide, determine the pH when: (a) 50.0 mL of base has been added. (b) 75.0 mL of base has been added. (c) 100.0 mL of base has been added.

40.00 mL of a 0.1000 M carbonic acid (H2CO3) was titrated with 0.2000 M sodium hydroxide....

40.00 mL of a 0.1000 M carbonic acid (H2CO3) was titrated with 0.2000 M sodium hydroxide. carbonic acid pka1:6.35 pka2:10.33 1.Calculate the volume of sodium hydroxide required to reach the first equivalence point. 2.Calculate the volume of sodium hydroxide required to reach the second equivalence point. 3.Write the balanced acid-base reaction and calculate the pH before the addition of sodium hydroxide. 4.Write the balanced acid-base reaction and calculate the pH after the addition of 12.00 mL of sodium hydroxide 5.Write...

A 25.0 mL sample of 0.100 M acetic acid is titrated with a 0.125 M NaOH...

A 25.0 mL sample of 0.100 M acetic acid is titrated with a 0.125 M NaOH solution. Calculate the pH of the mixture after 10, 20, and 30 ml of NaOH have been added (Ka=1.76*10^-5)

A 29.4 mL sample of 0.203 M ethylamine, C2H5NH2, is titrated with 0.237 M nitric acid....

A 29.4 mL sample of 0.203 M ethylamine, C2H5NH2, is titrated with 0.237 M nitric acid. At the equivalence point, the pH is ______.

A 27.7 mL sample of 0.314 M ethylamine, C2H5NH2, is titrated with 0.325 M nitric acid....

A 27.7 mL sample of 0.314 M ethylamine, C2H5NH2, is titrated with 0.325 M nitric acid. The pH before the addition of any nitric acid is . Use the Tables link in the References for any equilibrium constants that are required. kb: 4.3x10^-4

20.0 mL of 0.100 M copper(II) sulfate reacts with 20.0 mL of 0.100 M sodium hydroxide...

20.0 mL of 0.100 M copper(II) sulfate reacts with 20.0 mL of 0.100 M sodium hydroxide to form a precipitate (Cu(OH) 2 2 ). What is the concentration (molarity) of Cu 2+ in the resulting solution?

13.A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2....

13.A student mixes 100.0 mL of 0.500 M AgNO3 with 100.0 mL of 0.500 M CaCl2. a.Write the balanced molecular equation for the reaction. b.Write the net ionic equation for the reaction. c.How many grams of precipitate will form? d.What is the concentration of Ag+, NO3‒, Ca2+, and Cl‒ in the final solution (assume volumes are additive).

25.0 mL of a 0.100 M NH3 is titrated with a strong acid. 0.100 M HCl....

25.0 mL of a 0.100 M NH3 is titrated with a strong acid. 0.100 M HCl. Calculate the pH of the NH3 solution at the following points during the titration: (Kb= 1.8 x 10^-5) A. Prior to the addition of any HCl. B: After the addition of 10.5 mL of a 0.100 M HCl. C: At the equivilance point. D: After the addition of 3 mL of 0.100 M HCl. Show your work.

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