Question (1) The pH of an acidic solution is 3.45. What is [H⁺]?

Q: pH = %3D

A:

Q: 1. What species is the conjugate acid of HCO3? Write the formula and net charge. 2. Which species is…

A: 1. Conjugate acid of HCO3- is H2CO3. Net charge is zero.

Q: What is the hydroxide concentration in a solution with a pH of 12.57 at 25 oC?

A: Given pH = 12.57

Q: What is the pOH of a solution that has a pH of 9.9?

A: Here we have pH = 9.9 We have to find pOH .

Q: What is the pH of a solution with OH- of 0.00015 M KOH at 25°C. Give the answer in 2 significant…

A: Given :- concentration of KOH = 0.00015 M  To calculate :- pH of the solution  Nature if solution

Q: a) Determine the pH for the following solution: [OH−] = 1.6×10^−5 M  b) Is the above solution…

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Q: A common ketone starting material is shown below. Predict the major product for each reaction based…

A: Given that , An aldehyde reacts with different reagents and the respective products are as follows.

Q: Calculate the [OH-] of a solution at 25°C, if [H*] = 4.4 x 10-3 M. (answer in scientific notation)…

A: Given :- [H+]  = 4.4 × 10-3 M To calculate :- [OH-] at 25°C

Q: 1) A weak acid or a weak base ionizes completely.

A: A strong acid is defined as an acid which is ionized completely in an aqueous solution

Q: What is the pH of a 0.750 M solution of C,H,NHB (Kb of C,H̟N is 1.7 10°)?

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Q: Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric…

A: pH  of any solution = -log[ H3O+]Given in the question,pH of the solution = 4.240Molar concentration…

Q: What is the pH of 0.0988 M solution of NaOH? Enter answer into box rounded to two decimal places.…

A: Concentration of NaOH = 0.0988Mi.e. [HO-] = 0.0988 MpH = ?

Q: -The pH of a solution is 8.75. What is its [OH-]?)

A: pH= 8.75 [OH-] = ?

Q: What is the pH for a solution with [OH-] = 8.9 × 10-⁹ M? Respond with the correct number of…

A: Method 1:

Q: Calculate the pH and pOH of a solution at 25°C, if [H] = 2.6 x 10³ M. Answer to the hundredths…

A: 1) Given :-  [H+] = 2.6×10-3 (M)  pH = ?  pOH = 1  -----------------------------------------

Q: 4.55 pH what is the [OH-]

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Q: Q1 Complete the following table: [OH¯] pH [H,O*] Acidic, Basic, or Neutral? 2.0x10-6 9.8 3.5x10-3…

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Q: Question 6 Which compound is the weakest acid? O Bicarbonate ion (HCO3) O Formic Acid (HCOOH) O…

A: Explanation :

Q: ) Calculate the pH, [H+] and (OH-] of a solution with a pOH of 5.36 e) What is the pH of a solution…

A: Since you have posted question with multiple subparts as per guidelines we can answer three per…

Q: Calculate the concentration of OHminus if the pOH = 2.18. Report your answer in standard form not…

A: The relation between pOH and concentration of OH- is given as -…

Q: Question 6 For a base, the pH is 7. O equal to O less than O greater than

A: For a base , the PH is greater than 7.

Q: A solution has a pH of 5.38. (SHOW CALCULATIONS) a) What is the pOH? b) What is the hydronium…

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Q: The [H3O+] is 6.2x10-5 M; so, the [OH-] is 1.6x10-10.

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Q: Which of the following acids would be classified as monoprotic? Your answer: O A) sulfurous acid O…

A: We know that, Monoprotic acid are those acid which releases only 1 H+ ion in aqueous solution. i.e…

Q: A certain solution has a hydrogen ion concentration of 10 5.50 -8.50 8.50 -5.50 M, or [H+] = 10 .…

A: We know that pH is the negative logarithm of hydrogen ion concentration. That is  pH = – log[H+]

Q: 9) Calculate [H] in each aqueous solution at 25°C & classify solution as neutral, acidic or basic.…

A: Answer:- The solution which has higher hydrogen ion concentration than that of hydroxide ion…

Q: Which of the following is a characteristic of an base? has a pH above 7 all of the three bitter…

A: There are 2 types of species-  1- Acid 2- base

Q: Identify the following species as strong or weak acids or bases. a) HF b) NaOH c) NH3 d) HCIO4 e)…

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Q: 2. Calculate the [ H*] of each of the following given the pH and pOH a) pH = 2.5 b) pH = 5.2

A: Formula used pH = - log [H+] = 1[H+] = antilog (pH)

Q: Classify the compounds strong acids or weak acids. as Strong acid Weak acid Answer Bank H,SO, HNO,…

A: According to the Bronsted-Lowry concept of acid-base theory, the acids are proton donor and to…

Q: A mystery acid is discovered in a lab and only labeled as "Strong Acid!" To figure out the identity…

A: Given : The acid is a strong acid. Mass of acid dissolved = 5.00 g pH = 0.800 And volume of solution…

Q: 54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify…

A: Since, you have given multiple subparts, we will solve the first 3 subparts for you. For other parts…

Q: ||| SIMPLE RE Identifying acids and bases by their chemical formula Classify each chemical compound…

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Q: Question number 6 Calculate the concentration (molarity) of CH,NH, in a solution that is 0.0614 M…

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Q: Part A If 20.0 ml of 0.175 M aspirin (also known as acetylsalicylic acid), a monoprotic weak acid…

A: Part A-Given: 20 ml of 0.175 M aspirin (HC9H7O4) whose ionization constant  ka=3.00×10-4. The…

Q: 34 of 4 I Review | Constants Periodic Ta MISSED THIS? Read Section 17.7 (Pages 754 - 758) Part A For…

A: We will use formula of pH and pOH.

Q: 4. Complete the table below and answer the questions. For the Column 4, multiply [H+] and [OH-]…

A: pH is equal to the negative log of the hydronium ion concentration. pOH is equal to the negative log…

Q: What is the pH of a solution, having the H30 concentration of 0.0000000028 M? QUESTION 6

A: Given - - > [H3O+] =0.0000000028 M             OR [H3O+] = 2.8 x 10-9 M

Q: What is the pH of a 0.310 M ammonia solution? Express your answer numerically to two decimal places.…

A: Given;

Q: Part A Write the formula of the conjugate acid for base CO3. Express your answer as a chemical…

A: When a base is reacted with a proton (hydrogen ion), formation of conjugate acid takes place in the…

Q: if the pH of a 0.29 M aqueous solution of a weak base is 9.9, estimate the Kb of the base. Kb=?

A: pH= 9.9Concentration of weak base= 0.29M Kb=?

Q: A solution of NH3 and a solution of NaOH have the same pH. Which solution will require the most…

A: It is Based on the concept of neutralization reaction.  we need to identify the base which will…

Q: How many times higher is the [H† concentration in a solution with pH = 6 than a solution with pH =…

A: We know that PH= -log(H+)

Q: Questions: 1.Are food items such as juice or vinegar acidic or basic? What ion probably accounts…

A: (1) Food items like juice or vinegar are weakly acidic in nature. These have pH level less than 7.…

Q: Calculate the [OH-] of a solution at 25°C, if [H] = 9.6 x 101 M. (answer in scientific notation)…

A: The correct answer is given below

Q: Calculate the following:  a) [H+] and [OH-] of water with a pH of 7.2 b) [H+] and pH when [OH-] =…

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Q: 1) Indicate whether each solution is acidic, basic, or neutral: -4 a) 2 x 10 M OH b) 6 x 10 M H -10

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: 7) Decide whether each of the following will cause an aqueous solution to be acidic, basic, or…

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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.