Answered: What is the pH value of the solution…

What is the pH value of the solution formed by mixing equal volumes of a strong acid solution with a pH of 3 and a strong base solution with a pH of 12?

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.133E

See similar textbooks

Related questions

Q: What pH results when 0.75 mol of acetic acid is dissolved in enough water to make 3.0 litres of…

A: Acetic acid is a weak acid and will partially dissociates into its ion. Molarity is defined as the…

Q: If some NH4C1 is added to an aqueous solution of NH3: A) the pH of the solution will increase B) the…

A: The chemical reaction of an aqueous solution of ammonia is given below. NH3 + H2O ⇌ NH4+ + OH-. To…

Q: Define pH. What pH range is considered acidic? Basic? Neutral? (Assume 25 °C.)

Q: Does the pH of a solution increase or decrease when a strong acid like Hydrochloric acid (HCl) is…

A: We know the relation between the concentration of hydrogen ion and pH of solution→…

Q: What is the concentration of H3O+, in M, of a solution with a pH of 1.11?

A: Given : pH of Solution = 1.11 [ H3O+ ] = ? We know the following formula pH = - log[ H3O+ ]

Q: Q4 Which solution(s) showed the greatest change in pH? Why? Q5 Which solutions(s) showed little or…

Q: What is the pH of a solution composed of 1.0 x 10-6 M sodium hydroxide solution?

A: Acid is commonly sour. An acid is a substance that renders an ionizable hydronium ion (H3O+) in its…

Q: What is the pH of a solution that is 2.7×10-9 M in NaOH

Q: is the salt HONH3Cl acidic, basic, or neutral?

A: The salts that are formed from the strong acid - strong base are acidic salts. The salts that are…

Q: alculate the pH and the concentrations of all species in a 0.150 M Na2HPO4 solution.

A: Weak Acids are the acids that do not completely dissociate into their constituent ions when…

Q: What is the pH of a solution in which 46 mL of 0.14 M NaOH is added to 10. mL of 0.100 M HCl? pH =

A: In the reaction : HCl + NaOH -------> H2O + NaCl 1 mole of NaOH reacts With 1 mole of HCl…

Q: calculate the ph of an aqueous solution that contains 8.5x10-2 M hydroxide ion

Q: What is the pH of a solution if 10 mL of 1.0 M HCl is added to 10 mL of 3.0 M NaOH solution?

Q: A solution in which [H+] = 10-3 M is whereas a solution in which [H+] = 10-10 M is +. Give the pH…

Q: Explain the difference between a strong acid and a weak acid?

A: Strong acid – It is defined as an acid completely dissociate in its aqueous solution is called as…

Q: Solution 1 has [H+] = 8.6×10-7 M, and solution 2 has [H+] = 8.6×10-4 M. Calculate pH of both…

A: pH is given by the equation pH = -log [H+] where [H+] = concentration of H+ ions present in the…

Q: What is the pH of a solution with a hydroxide ion (OH-) concentration of 10-10M?

A: pH is related to pOH by the following expression: pH + pOH = 14 ⋯⋯⋯⋯(1) Also pOH is related to the…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: Salt of strong acid and weak base = Acidic salt Salt of weak acid and strong base = basic salt Salt…

Q: The pH of a basic solution is 11.99. What is [H⁺]

A: pH of the solution is defined as "the negative logarithm to the base 10 of the value of the…

Q: What is the pH of a 4.21 x 10-5M KOH solutio

A: pH helps in the measurement of acidity and basicity of a solution.

Q: Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral. compound…

A: The nature of aqueous solution of given salts depends on nature of acid and base given .

Q: List the acidic salts in increasing order of acid strength, then list the basic salts in increasing…

A: Acid are the substance which donates proton in the aqueous solution. Example:HCl(aq)→H+(aq)+Cl-(aq)…

Q: A solution of an unknown chemical has a pH of 9. Is this solution acidic or basic?

A: Given A solution of an unknown chemical has a pH of 9.

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: A mixture of weak acid and its salt forms a buffer solutions or buffers. Buffers solutions resist…

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCI with 40.00 mL of 0.10 M KOH?…

A: It is an example of acid base neutralisation reaction in which an acid is neutralises by the base…

Q: What is the percent ionization of an acid? Explain what happens to the percent ionization of a weak…

A: The percent ionization is the comparative ratio of the ionized acid’s concentration to the initial…

Q: 1. Which is the pH of 1M NAOH solution? 2. Which is the pH of 1M HCI solution? 3. Which is the pH of…

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

Q: What is the pH of a solution obtained by adding 222 mL of 0.111 M HCl to 596 mL of a HNO3 solution…

A: Since both HNO3 and HCl are strong acids Hence they will dissociate completely in solution Hence…

Q: How is calculating pH of a salt different than a calculating pH of a weak acid or base ?

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

Q: What is the pH of a solution formed by mixing two equal volumes of solutions of HCI, one with a pH…

A: pH = - log [H+] - pH = log[H+] [H+] = 10-pH

Q: What is the ratio of acid to base in a solution having a pH=9?

A: Assume pKa of acid = 8.5

Q: What is the pH of a solution that has a hydrogen ion con- centration of 1.0 X 10 M? 46. TATI

Q: A solution increases the OH^- ion concentration of another solution Does the property describe a…

A: Please move to 2 step to get answer of your question Thank u

Q: The pH of a solution prepared by mixing 2.0mL of a strong acid solution of pH 3.00 and 3.0mL of a…

A: The pH of resulting solution can be calculated as follows

Q: Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral. compound…

A: On the pH scale whose pH is less than 7 is said to be acidic and whose pH is greater than 7 is said…

Q: Water with a pH value (less, greater) than 7 is basic.

A: PH value: pH value is a mathematical value used in the identification of the acidic and basic nature…

Q: Hydrochloric acid, HCl, completely ionizes when dissolved in water. Calculate the pH of a solution…

A: pH is considered the negative log of the hydrogen ion concentration and it is represented by moles…

Q: The pH of a basic solution is 9.23. What is [H⁺]?

A: pH can be calculated by a general formula i.e. pH = -log [H+]

Q: What is the pH of a solution in which 43 mL of 0.33 M NaOH is added to 13 mL of 0.170 M HCl?

A: Moles of NaOH and HCl are determined as follows,

Q: A solution contains electrolytes Does the property describe a solution that is acidic , basic , both…

A: Electrolytes are those substances which dissolved in water to produce cations and anions. Generally,…

Q: What is the final pH of the solution when 10 mL of 0.1 M NaOH is added to 50 mL of 0.05 M HCl…

Q: What is the pH of a solution in which 15 mL of 0.15 M NaOH is added to 25 mL of a 0.10 M HCl ?

A: HCl is a strong acid and NaOH is a strong base. The net ionic equation involved in the titration of…

Q: The pH of a 0.10 M solution of a weak base is 9.67. What is the Kb of the base?

A: Assuming the weak base is monoprotic base Hence the dissociation of base will have below reaction…

Q: What is the pH of a solution obtained by adding 219 mL of 0.309 M HCl to 905 mL of a HNO3 solution…

A: We have given that Concentration of HCl = M1 = 0.309 M Volume of HCl = V1 = 219 mL Volume of HNO3…

Q: Indicate whether the salts below would form solutions that are acidic, basic, or neutra in pH.…

Q: What is the pH of a solution in which 15 mL of 0.16 M NaOH is added to 25 mL of 0.16 M HCl? pH =

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: NH₄Br It is made of a strong acid (HBr) and weak base (NH3).

Q: A solution having a pH of 7.85 is:

A: If pH<7 then solution is acidic in nature pH =7 then solution is neutral pH>7 the solution is…

Q: The pH of a weak base (B) is 9.99 when the concentration of the weak base is 0.18 M. What is the…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

What is the pH value of the solution formed by mixing equal volumes of a strong acid solution with a pH of 3 and a strong base solution with a pH of 12?

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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

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

What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
Explain the difference between a strong acid and a weak acid.
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.
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
A buffer solution has a pH value of 9.8. Which value in the set of pH values 8.79.79.89.910.9 is the most likely value for the buffer solution pH after a. a small amount of strong acid has been added? b. a small amount of strong base has been added?
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
In Arrhenius acidbase theory, what ion is responsible for the properties of a. acidic solutions b. basic solutions
When might a pH meter be better than an indicator to determine the end point of an acid-base titration?
Four different substances of the generalized formula HA were dissolved in water, with the results shown in the diagrams. Which of the diagrams represents the substance that is the strongest electrolyte?
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the following acids? More than one term may apply in a given situation. a. H3PO4 b. H3PO3 c. HBr d. HC2H3O2
Classify each of the following compounds as a strong electrolyte or a weak electrolyte. a. H3PO4 b. HNO3 c. KNO3 d. NaOH