The pOH of a solution is 9. Which of the following is correct? (A) The solution is basic with an [OH] of 1 x 10-5 M (B) The solution is acidic with an [H*] of 1 x 10-5 M (C) The solution is basic with an [OH] of 1 x 10 M (D) The solution is acidic with an [H*] of 1 x 10

Q: The pOH of a basic solution is 3.03 what is the [OH-]?

A: Given :- pOH of basic solution = 3.03  To calculate :- concentration of OH- ions i.e. [OH-]

Q: 7. The [OH-] of a solution is 1 x 10-2 M. Which of the following is correct? (A) The solution is…

A: Given,  The concentration of OH- , [OH-] = 10-2 M We know that, pOH = - log [OH-]  pOH + pH = 14…

Q: the Ph of a 0.050 M weak acid solution is 5.25. Calculate the Ka of the acid.

A: Given, pH of weak acid= 5.25 [weak acid ] =0.050 M Ka = ?

Q: Calculate the pH and the pOH of 0.78M NaOH

A: NaOH(aq) ---------> Na+ (aq) + OH-(aq) 0.78 M NaOH will give 0.78 M Na+ ions and 0.78 M OH- ions.…

Q: The pH of a 0.0058 M solution of HNO, is

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

Q: Calculate [OH-] for each of the following solutions, andindicate whether the solution is acidic,…

A:

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: Which of the following is not a strong acid? O HNO3 O H2S04 O HCIO4 O H3PO4 OAll are strong acids.

A: The acids which dissociates completely or ionized in aqueous solution are known as strong acids.…

Q: The pOH of a basic solution is 2.65. What is PH?

A: Given, the pOH of a basic solution, pOH =2.65we are asked to calculate the pH of the solution.

Q: The pOH of a solution is 9. Which of the following is correct? (A) The solution is basic with an…

A: Given  POH  = 9  Nature of solution  = ?

Q: The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39. What is the Ka of the acid?

A: pH is the universal indicator , that not only help in detecting the acidic/ basic character but also…

Q: The substance HIO3 is expected to be a stronger acid than the substance HIO.

A: Acidity depends on the oxidation state of central atom.

Q: The pOH of a basic solution is 2.87. What is pH?

A: We have given that  pOH = 2.87  We know that  pH + pOH =14  pH = 14 - pOH        = 14 - 2.87   pH =…

Q: The pH of a 0.0042 M solution of HNO is

A:

Q: A 0.050 M solution of a weak acid (HA) has a pH of 4.70. What is the Ka of the acid?

A: We will have the below reaction taking place. HA ----> H+ + A- Since pH = -log[H+] where [H+] =…

Q: ph level of  NH4OH, HFO, HIO4, Be(OH)2

A: We have to level the pH of the following NH4OH, HFO, HIO4, Be(OH)2

Q: The pOH of a basic solution is 3.83. What is [OH]?

A: For basic solutions calculation of POH formula  POH= - log[ -OH]  Calculation of [ -OH]  formula  […

Q: The pH and pOH of 0.05 M of NaOH is ..

A:

Q: Calculate the [OH in a solution that has a pH of 2.92.

A: We know that, pH can be expressed as negative logarithm of H+. i.e.,                      pH = -…

Q: If the pH of a 2.54-cm rainfall over 4600 km is 3.50, how many kilograms of sulfuric acid, HSO4, are…

A: Given: pH of acid rain = 3.50 height of rainfall = 2.54 cm Area of rainfall = 4600 km2

Q: Determine the pH of a 0.500 M HA solution if the Ka of H

A: Welcome to bartleby !  Introduction :  We have to calculate pH .

Q: What is the pH of the following solution. 0.035 M HNO3

A: Given data contains, Molarity of nitric acid is 0.035 M.

Q: The pOH of a basic solution is 3.99. What is pH?

A: Given :- pOH = 3.99 To be calculated :- pH of the solution

Q: The pOH of an acidic solution is 11.55. What is [OH 1?

A: The pOH of the solution is = 11.55 The hydroxide ion concentration of the solution is =?

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: The pH of a 0.0046 M solution of HNO, is

A: Ph is the negative logarithm of the concentration of Hydrogen ion for dilute solutions. Thus, pH is…

Q: The pOH of a basic solution is 3.47. What is [H*]?

A: Given data, pOH = 3.47 To calculate the [H+].

Q: The pH of an aqueous solution of 1.00 x 10-2 M HOCN is 2.77 at 25 0C. Calculate Ka for HOCN

A: Given pH = 2.77 Concentration of HOCN = 1×10-2 = 0.01M

Q: What is the pH of a solution that has [OH–] of 5.15×10-3 M ?

A: Given, Concentration of hydroxide ion = 5.15×10-3 M

Q: The pOH of a basic solution is 5.99. What is [OH¬]?

A: Given :- pOH = 5.99  To be calculated :- [OH-]    pOH = - log[OH-]

Q: calculate the ph of the following solution and tellw hether it is acidic, basic, or neutral…

A: Given, [H3O+] = 4.53 ×10-8 M

Q: you prepare a solution of 3.1 x 10-8M KOH and calculate the pH in the typical way for a strong base:…

A: Molarity Of KOH solution = 3.1 * 10-8 M Calculated pOH = 7.51 Calculated pH = 6.49 pH recorded by pH…

Q: If the pH of a 0.55 M solution of acid is 5.4, what is the KA?

A:

Q: Which one of the following molecules is a strong acid? Select one: o Ca(OH), O HF O NH, HClo,

A:

Q: Which of the following statements is/are true? (Select all that apply) OThe higher the concentration…

A:

Q: The pH of a solution of 0.50 M  NH4Cl  is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: Calculate the pH of a 0.20 M solution of HCN, which has a Ka of 4.9×10-10 at 298 K.

A: Given  0.20 M solution of HCN, which has a Ka of 4.9×10-10 at 298 K. pH has to be determined for…

Q: With the information given, determine pH of the following solutions and indicate if they are…

A:

Q: What is the concentration of hydronium ion H3O+ in a solution with a pH -1.3?

A: pH of any solution is given by  pH = -log[H3O+ ]  where [H3O+ ] = concentration of hydronium ion

Q: Write a net ionic equation to show that ascorbic acid, H2C6H6O6, behaves as an acid in water.…

A:

Q: When lithium oxide (Li2O) is dissolved in water, the solutionturns basic from the reaction of the…

A: According to Arrhenius concept, bases are those that can release OH- ions in aqueous solution. When…

Q: Which of the following salts are basic?     LiF     NaClO4      C6H5NH3I…

A: For the given compounds, the aqueous solution of salt, such as KNO3 and NaClO4 is neutral because it…

Q: Given the pOH is 12.22 a. what is [H+] b. what os [OH-] c. is it acidic or basic?

A: a. The relationship between the hydronium ion concentration and the hydroxide ion concentration is…

Q: A truck transported 400 liters of HCl approximately 7.4M a) Is it a strong or weak acid? b) What is…

A: According to the Arrhenius theory, the substance that gives hydrogen ion H+ in the aqueous solution…

Q: Calculate the pH of a solution if it's OH = 0.0800M Is this solution basic or acidic?

A: Recall the following relations            pOH=-logOH-          pH+pOH=14If value of pH for a…

Q: The pOH of a basic solution is 3.67. What is pH?

A:

Q: give the formula of the conjugate acid of HSO4-

A: Conjugate acid: Bronsted-Lowry Base that accepts proton result in protonated base is known as…

Q: Which of the following is acting as an acid? CH3COOH + NH3 CH3COO + NH4+ CH;COOH O NH3 NH, O CH;COO

A: Bronsted-Lowry acid-base theory: According to the Bronsted-Lowry acid-base theory, acid is 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.