Can you help me plz thankyou so so much 5. If 30 ml of a 0.58M solution of HF is reacted with 25 ml of a .65M solution of NaOH, whatis the resulting pH?1 HF1 NAOH->1 NaF1 H206. If 80 ml of a .35M solution of HCIO; is reacted with 90 ml of a .30M solution of LIOH, what1 H2Ois the resulting pH?1 HCIO31 LIOH->1 LICIO;

Answered: 5. If 30 ml of a 0.58M solution of HF…

5. If 30 ml of a 0.58M solution of HF is reacted with 25 ml of a .65M solution of NaOH, what is the resulting pH? 1 HF 1 NaOH -> 1 NaF 1 H20

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 40P

See similar textbooks

Related questions

Q: A 0.125 M solution of HNO2 has a pH = 2.08. What is Ka for HNO2?

A: Answer) HNO2 is weak acid . When we dissolved it in water it give H+ ions. It does not dissolve…

Q: What is the [OH] in a solution with a pH of 9.22? (1.7 X 10 M)

A: Given that pH of solution=9.22

Q: A solution of Mg(OH)2 was found to have a pH of 12.64. Determine the initial concentration of the…

Q: White vinegar has a pH of 2.4 while apple cider has a pH of about 4.25. What is the difference…

Q: A solution has a pOH of 6.50 at 50∘C. What is the pH of the solution given that Kw=6.22×10−15 at…

A: To determine pH of solution: First we have to calculate pKw,

Q: calculate the pH of solutions with the following hydronium ion concentrations a. 1.00 x 10^9 MH3O+…

A: To calculate the pH of a solution,we use the following Equation, pH = - log[H3O+] a) For 1.00 x…

Q: (a) What is the pH of 0.65 M potassium formate, HCOOK? (b) What is the pH of 0.85 M NH4Br?

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: The pH of a white vinegar solution is 2.20. This vinegar is an aqueous solution of acetic acid with…

A: Concentration of H+ can be calculated as follows:

Q: 15.18/Calculate the pH of each of the following solutions: (a) 2.8 x 10 M Ba(OH)2, (b) 5.2 x 10 M…

Q: What is the pH of a 0.00065 M solution of HI?

A: The pH of the solution has to be calculated,

Q: A 4.9 × 10−3−mol sample of HY is dissolved in enough H2O to form 0.090 L of solution. If the pH of…

A: given, number of moles of HY = 4.9 × 10−3 Volume of solution = 0.090 L the pH of the solution = 2.55

Q: 4. A certain brand of rootbeer has a hydrogen concentration equal to 1.9 x 10 M. What is the pH and…

A: pH =-log[H+] pOH = -log[OH-]

Q: A) What is the concentration of PO43- in a 0.18 M H3PO4 solution? Ka1= 7.5X10-3 , Ka2=6.2X10-8,…

A: a) The concentration of phosphate ion is calculated as,

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: What is the pH of a 1.00 molar solution of NH4Cl(aq)? The Kb for NH3 = 1.8 × 10–5 .

A: Ammonium chloride dissociates completely into ammonium and chloride ions. The ammonium ion is the…

Q: (a) What is the concentration of the Acid? D.l [=Mores しLQrs ミ 20 O.005 BasE PL (b) What is the pH…

A: (a) Reaction between NaOH and H2CO3…

Q: What is the pH of IxE-9 M HCI solution? O a. 6.99 O b. 9.00 Oc. 9.1 O d. 7.5

A: Answer: option b. 9.00 is the pH of the HCl solution.

Q: 2. If the [H'] in a certain tap-water sample is 2.6x107 M, what is the OH° concentration? Determine…

A: Answer 2 : Given : [H+] = 2.6 × 10-7 M [OH-] = ? pH = ?

Q: The molarity of an aqueous solution of NaOH is 0.0022 M. (a) What is the concentration of H3O+ in…

Q: What is the pH of a 4.7 × 103 M HI solution?

Q: 35. What is the pH of the resulting solution when 0.20 mol of HCl is added to 0.250 L of water?

Q: 5.02

A: This question is related to pH.

Q: The pH of a white vinegar solution is 2.28. This vinegar is an aqueous solution of acetic acid with…

Q: 11. What is the pH of a 0.00065 M solution of HI? 3.2 6.5 O 10.8

A: The complete reaction ; HI ⇔ H+ + I- Concentration of HI = 0.00065 M

Q: An unknown solution has a pH of 7.2. Which of these chemicals is likely to cause the greatest…

A: given data pH = 7.2

Q: a) What is the concentration of a solution prepared by mixing 35.0 mL of o.10 Macetic acid with 15.0…

A: a) Given : Concentration of acetic acid i.e HC2H3O2 taken = 0.10 M Volume of HC2H3O2 solution taken…

Q: The pH of a household cleaning solution is 11.17. This cleanser is an aqueous solution of ammonia…

A: Given, pH = 11.17 Density = 1.00g/mL Kb = 1.8*10-5

Q: Express the pH of the solution to three decimal places. 0.300 g of HClO3 in 2.9 L of solution

A: The pH of the given solution is to be determined to three decimal places- 0.300 g of HClO3 in 2.9 L…

Q: calculate the pH of each of the following strong acid solutions: a. 8.5*10^-3 M HBr b. 1.52 g…

Q: A solution has an OH⁻ concentration of 1.3 x 10⁻⁴. What is the pH of the solution at 25°C?

A: pH = -log [H+] [H+][OH-] = 1 x 10-14 at 25°C

Q: The pain reliever codeine is a weak base with a Kb equal to 1.6×10–6. What is the pH of a 0.250 M…

A: Let the general formula of the weak base be BOH. It will dissociate as:…

Q: 4.7 What is the pH of each solution? a) 2.2 × 10-2 M HNO3 b) 1.05 М HI f) o.52 M KOH

A: Calculate the pH of given solutions a HNO3 = 2.2×10-2M b 1.05M HI f 0.52M KOH

Q: Methylamine, CH3NH2, has Kb= 4.4 x 10–4. (a) Write the ionization equation of methylamine in…

A: Ionization reaction is defined as the reaction in which a chemical specie gains or loses electrons…

Q: How many moles of nitric acid do you have in a 0.650 L solution of 0.035 M nitric acid? What is the…

A: Given Data : Nitric acid molar conc. = 0.035 M Volume of nitric acid = 0.650 L Mole of nitric acid…

Q: 21) a 10.0 mol sample of HCl is mixed with 5.0 mol sample of NH,OH in 150.0 milliliter solution,…

A: Following information given in the question - Moles of HCl in Solution = 10 moles Moles of NH4OH…

Q: The pH of 750 mL (3 SF) of an aqueous solution containing only NaNO 2 is 8.42. If HNO 2 has a Ka of…

Q: Calculate [OH-], pOH, and pH for each of the following. a. 00040 M Ca(OH)2 b. a solution containing…

Q: Calculate the pH of a solution made by adding 2.70 g of lithium oxide (Li2O) to enough water to make…

A: Mass of lithium oxide = 2.70 g Volume of solution = 1.300 L

Q: (a) What is the pH of 0.65 M potassium formate, HCOOK?(b) What is the pH of 0.85 M NH₄Br?

A: pH is defined as the minus of the logarithm of hydrogen ion concentration([H+]). That is(i.e.),…

Q: NaOH is a strong electrolyte, so the value of OH- comes from the strong electrolyte.Calculate the pH…

A: pH is a scale which measures the acidity or basicity of the given aqueous solutions. Mathematically,…

Q: 4. If you had 98 ml of a .60M solution of HCN that you mixed with 110 ml of a 0.50M solution of KOH,…

Q: What is the pOH of a solution that has a pH of 3.4?

Q: Exactly 250 ml solution was made by dissolving 0.01 g of NaOH in water. What is the PH for the…

Q: What is the concentration of H+ in moles/L in a solution that has a pH of 8.35?

A: Given :- pH of solution = 8.35 To calculate :- concentration of H+ ion (mol/L)

Q: A generic base, B, is added to 40.00 L of water. The pH of the solution is found to be 9.00. What is…

Q: 1.Why does the autoionization of water occur? 2.What is the definition of a strong acid? The…

A: Note - Since you have posted a question with multiple sub-parts, we will solve the first three…

Q: What is the pH of a solution if 10mL of 0.1 M HCl is added to 10mL of 3.0 M NaOH solution? a) 7 b)…

Q: Hypobromous acid, HBrO, can be produced commercially as a disinfectant. A solution is made by…

A: HBrO is a weak acid. pH = -log[H+] For a weak acid solution: [H+] = (Ka x C)1/2 Where, C = molar…

Q: mol

A: First we will calculate, amount of H+ ions in solution. pH = -log[H+] [H+] = antilog(-pH). [H+] =…

Concept explainers

Environmental Pollution

Environmental pollution occurs due to some unwanted alteration in the surroundings which results in unfavorable effects on all organisms of that surrounding.

Question

100%

Can you help me plz thankyou so so much

5. If 30 ml of a 0.58M solution of HF is reacted with 25 ml of a .65M solution of NaOH, what
is the resulting pH?
1 HF
1 NAOH
->
1 NaF
1 H20
6. If 80 ml of a .35M solution of HCIO; is reacted with 90 ml of a .30M solution of LIOH, what
1 H2O
is the resulting pH?
1 HCIO3
1 LIOH
->
1 LICIO;

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1 Balanced reaction

VIEW

Step 2 Caluclation

VIEW

Step 3 Conclusion

VIEW

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Calculate the pH of a solution prepared by mixing 49.0 mL of butyric acid, HC4H7O2, with 6.15 g of KOH in water. The following data about butyric acid may be helpful: density=0.9595g/mL;K a =1.54105
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
At 25 C, a 0.10% aqueous solution of adipic acid, C5H9O2COOH, has a pH of 3.2. A saturated solution of the acid, which contains 1.44 g acid per 100. mL of solution, has a pH = 2.7. Calculate the percent dissociation of adipic acid in each solution.
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
Water is accidentally added to 350.00 mL of a stock solution of 6.00 M HCI. A 75.00-mL sample of the diluted solution is titrated to pH 7.00 with 78.8 mL of 4.85 M NaOH. How much water was accidentally added? (Assume that volumes are additive.)
Is the conjugate base of a weak acid a strong base? Explain. Explain why Cl does not affect the pH of an aqueous solution.
How many grams of HI should be added to 265 mL of 0.215 M HCI so that the resulting solution has a pH of 0.38? Assume that the addition of HI does not change the volume of the resulting solution.
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.