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

Q: type of compound (check all that apply) compound ionic molecular acid base HBrO, H, PO4 H, SO, H,…

A: If the compound is only formed by ionic bond , than that is called ionic compound. If the compound…

Q: If a solution has pH of 5.50, calculate its [OH-]*

A: Given  PH = 5.50  [OH- ]  = ?

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 solution of NaOH has a concentration of 0.104 M. What is the pH of the solution? Report your…

A: Answer:- This question is answered by using the simple concept of calculation of pH of a strong base…

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

A:

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: ydrogen ion concentration of a solution with pH = 12.75?

A: pH is equal to negative logarithmic of hydrogen ion concentration

Q: If the pH of a solution is 1.78, what is the concentration of [H+]?

A: pH = -log [H+]

Q: Calculate the pH of solutions having the following  [H+]: a) 0.0020 M b) 7.0 x 10(-8) M c) 3.0 M

A:

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

A:

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: Calculate the concentration of H3O+ if the pH of a solution is 2.19. Answer to two significant…

A:

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: Given a solution in which the pH = 4, determine [H+], [OH-] and pOH.

A: Inorganic chemistry.

Q: What is the pH of a 0.0550 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-1⁰)?

A:

Q: The pH Of An Unknown Solution Is 0.46. Calculate [H3O+] In Solution.

A:

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

A:

Q: b Calculate the pH of the following solution from the information given: РОН - 4.75 pH =

A: Answer:- this question is answered by using the simple concept of calculation of pH using the value…

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

A: Explanation :

Q: For each of the following substances, predict the pH when each is dissolved in water.  If more…

A: When a salt is allowed to dissolve in water, then the salt will dissociate and reacts to form a new…

Q: What is the pH of 0.0035 M NaOH?

A: NaOH is a strong base which dissociates completety in solution.The dissociation equation of NaOH is…

Q: 2. Compare the concentration of the hydroxide ion to the hydronium ion in the type of solutions…

A: To Compare the Hydronium ion Concentration [H3O+] and Hydroxide ion concentration :

Q: what is the [OH^-] for a solution with a pH of 13.7.  answer in decimal form

A: Given that: pH = 13.7 pH = -log[H+]

Q: The pH of a basic solution is 12.83. What is [OH ]?

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

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: Construct the expression for Ka for the weak acid, NH,. NH, (aq) + H,0(I) = H;O*(aq) + NH(aq) Based…

A: Dissociation constant for acid, ka, is defined as ratio of product of concentration of products to…

Q: If the pH of a solution is 1.50, what is the concentration of [H+]?

A: pH of a solution is 1.50 We have to find the  concentration of [H+] We know that  pH = - log [H+]

Q: Determine the [OH-] in a solution with a pH of 4.358.  Your answer should contain 3 significant…

A: The relationship between the pH and [OH-] is given by  pH = 14 + log[OH-]  where [OH-] =…

Q: What is the pH of a 0.360 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?

A: concentration of NaCN = 0.360 MKa of HCN = 4.910-10Kw = 1.010-14

Q: A solution where [H⁺] = 1.0 x 10⁻¹³ M is ______________. A) strongly acidic B) basic C) neutral D)…

A: the correct option is as follows:

Q: Calculate [H3O+]and [OH−]or each of the following solutions at 25 ∘C given the pH pH=8.76 pH= 11.29…

A: pH is used to determine the concentration of hydronium ion . The expression for the pH is shown…

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: At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What…

A: 1. Extent of ionization of HNO2 = decreases  2. The concentration of H+ ion = decreases  3. The pH =…

Q: ph=2.81 what is the h+

A: Given,  The pH of the solution is 2.81  The hydronium ion (H+ ) concentration is:

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: An unknown weak acid with a concentration of 0.510 M has a pH of 5.600. What is the Ka of the weak…

A:

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

A:

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

A: [H3O+] [-OH] pH Acidic , basic , Neutral 2.0 * 10-6           9.8     3.5 * 10-3…

Q: Calculate the [H-] and identify if its acidic, basic or neutral.  pH= 4.6

A:

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.