Question

In: Chemistry

3. Find the pH of… A) 0.0055 M HBr B) 5.00 ml of LiOH after it...

3. Find the pH of…

A) 0.0055 M HBr

B) 5.00 ml of LiOH after it is diluted to 500 ml

C) 2.00 M sodium benzoate (Kb = 1.5 x 10 ^-10)

E) Identify as acidic, basic or neutral:

KNO₃ NaF NH₄Cl

Expert Solution

pH = - log [H+]

A) 0.0055 M HBr

[HBr] = [H+]= 0.0055 M

pH = - log [H+] = - log [ 0.0055] = 2.26

Therefore,

pH of 0.0055 M HBr = 2.26

B) Molarity of LiOH is required to calculate the pH.

C) Given that

[sodium benzoate] , C = 2.00 M

Kb = 1.5 x 10^-10

We know that pOH = [-logKb- logC]/2

= [-log(1.5 x 10^-10)- log(2)]/2

= 4.76

pOH = 4.76

Then, pH = 14- pOH = 14- 4.76 = 9.24

Therefore,

pH = 9.24

E) a) KNO₃ = Neutral

KNO3 is formed from strong base KOH and strong acid HNO3. Hence, KNO3 is neutral.

b) NaF = basic

NaF is formed from strong base NaOH and weak acid HF. Hence, NaF is basic.

c) NH4Cl = acidic

NH4Cl is formed from weak base NH3 and strong acid HCl. Hence, NH4Cl is acidic.

queen_honey_blossom answered 2 years ago

Calculate the pH after adding 5.00 mL of 0.15 M HNO3 to 250 mL of an...

Calculate the pH after adding 5.00 mL of 0.15 M HNO3 to 250 mL of an acetic acid/acetate buffer with an initial pH of 4.32 and a total buffer concentration of 0.25 M. Neglect activity coefficients for this problem.

Consider the titration of of 5.00 mL of 0.450 M HBr using 0.120 M NaOH as...

Consider the titration of of 5.00 mL of 0.450 M HBr using 0.120 M NaOH as the titrant. a)Calculate the volume of 0.120 M NaOH that must be added in order to reach the equivalence point. b)Determine the pH of this titration solution at the equivalence point. c)Calculate the pH of this solution after 20.00 mL of 0.120 M NaOH has been added.

(50 mL of 0.02000 M KOH Titrated with 0.1000M HBr) Calculate pH after adding the following...

(50 mL of 0.02000 M KOH Titrated with 0.1000M HBr) Calculate pH after adding the following volumes of the titrant: (a) 3 mL (b) 10 mL (c) 10.5 mL Answers: (a) pH =12.12; (b) pH = 7.00; (c) pH = 3.0. I need a step-by-step explanation on how to do this.

1. Ph of H3O+ of 5.7x10^3 2. Ph of a 1.5x10^-2 m for HBr 3. ph...

1. Ph of H3O+ of 5.7x10^3 2. Ph of a 1.5x10^-2 m for HBr 3. ph of 3.24x10^-4 m of hypochlorous acid ka2.9x10^-8

After mixing 5.00 mL of the 5.0×10–5 M crystal violet solution with 5.00 mL of 0.20...

After mixing 5.00 mL of the 5.0×10–5 M crystal violet solution with 5.00 mL of 0.20 M NaOH, what is the concentration of crystal violet and hydroxide ions in the solution at the start of the reaction? Is it a reasonable assumption that the concentration of OH– is much greater than that of CV+? Why is this an important assumption? Explain.

1. Calculate the pH during the titration of 25.00 mL of 0.1000 M LiOH(aq) with 0.1000...

1. Calculate the pH during the titration of 25.00 mL of 0.1000 M LiOH(aq) with 0.1000 M HI(aq) after 24.2 mL of the acid have been added. 2. Calculate the pH during the titration of 30.00 mL of 0.1000 M CH3CH2COOH(aq) with 0.1000 M LiOH(aq) after 12 mL of the base have been added. Ka of propanoic acid = 1.3 x 10-5. Please help these questions!

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH...

A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH. Express your answer numerically. A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 15.0 mL of HNO3. Express your answer numerically. A 52.0-mL volume of 0.35 M CH3COOH (Ka=1.8×10−5) is titrated with 0.40 M NaOH. Calculate the pH after the addition of 33.0 mL...

3. What is the pH of the resulting solution after 150 mL of a 3.2 M...

3. What is the pH of the resulting solution after 150 mL of a 3.2 M sodium hydroxide solution is mixed with 4.0 mL of a 4.0 M vinegar solution? 4. In the above question is the acid or base a limiting reagent? 5. Calculate the pH after adding 40.0 mL of 3.7 M potassium hydroxide to 20.0 mL of 12 M formic acid. 6. How many more mL of the 3.7 M potassium hydroxide solution must be added to...

Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the...

Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added. Va = 0 mL Va = 1.0 mL Va = 5.0 mL Va = 9.0 mL Va = 9.9 mL Va = 10.0 mL Va = 10.1 mL Va = 12.0 mL Make a graph of pH versus Va = 0, 1.0, 5.0, 9.0, 9.9, 10.0, 10.1, and 12.0 mL.

A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x...

A student mixes 5.00 mL of 2.00 x 10‐3 M Fe(NO3)3 with 5.00 mL 2.00 x 10‐3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN+2 is 1.40 x 10‐4 M. What is the initial concentration in solution of the Fe+3 and SCN‐? What is the equilibrium constant for the reaction? What happened to the K+ and the NO3‐ ions in this solution?