The hydronium ion concentration of a solution is 3.8 x 10–2 M (3.8e-2). What are the pH, pOH, and hydroxide ion concentration? pH: pOH: [OH-]:

Q: What is the equation for calculating pH when given ( H30+) b. what is the equation for calculating…

A: The term pH of the solution is a measure of the acidity or the basicity of a given solution. More…

Q: The hydroxide ion concentration of a solution is 1.6 x 10–3 M (1.6e-3). What are the pOH, pH, and…

A: Given : [OH-] =1.6 x 10–3 M

Q: In a sample of lemon juice, H+ concentration is 3.8 x 10-4 M. What is the pH?

A: we know pH = −log [H+] where   [H+]  = concentration of H+

Q: How to Calculate [OH-] from pOH.

A: pOH is negative logarithm of [OH-]

Q: hat is the hydronium ion concentration in an aqueous nitric acid solution that has a pOH of 12.110?…

A: In the given question we have to calculate the hydronium ion concentration in aqueous in nitric acid…

Q: The pH of a 0.205 M solution of a weak acid, HB, is 2.58. What is K, for the weak acid?

A: The given data is as follows: The pH of solution = 2.58 The concentration of weak acid, HB = 0.205 M…

Q: The pH of a 0.551 M solution of sodium methanoate, HCOO°Nª*, is 8.75. Calculate K, for the…

A: Concentration of HCOO-Na+ = 0.551 M pH of the solution = 8.75

Q: Find the [OH-] in an acidic solution where [H+] = (6.0x10^-5)

A: An acid is a molecules which can donates protons or they are capable of donating hydrogens. Bases…

Q: The pH of an aqueous solution that contains 3.4 x 10-2 M NaOH is What is the pOH? Circle one: ACID…

A: Answer :- 1) i) pOH = 1.47  ii) the given aqueous solution is a Base.…

Q: At 25 °C, a solution has a hydronium ion concentration of 3.20x10-8 M. What is the pH, pOH, and…

A: The given data: The concentration of hydronium ions [H3O+] = 3.20×10-8 M To determine= pH, pOH and…

Q: Calculate the pH and pOH of the solutions with the following hydrogen ion or hydroxide ion…

A: The formula used for calculation of pH = -log [H+]

Q: At 25 °C, a solution has a hydronium ion concentration of 6.10×10-6 M. What is the pH, pOH, and…

A:

Q: The hydronium ion concentration of a solution is 3.5 x 10–9 M (3.5e-9). What are the pH, pOH, and…

A: The pH is the concentration of H+ ion in the solution. It can tell us if the solution is acidic or…

Q: Given the pOH for a solution, calculate the other values:   pOH = 5.33   a)   pH =  b)   [H3O+] =…

A: POH=5.33PH=-log H3+O                  POH=-log OH-10-PH=H3O+                     10-POH=OH-a PH=?…

Q: In an aqueous solution the  [OH-] is 1.0 x 10- 6 M. What is the [H+]

A: At 25oC, the mathematical relation between molarities of H+ and OH- is given as: [H+][OH-]=1.0×10-14…

Q: The pH of a 0.206 M solution of a weak acid, HB, is 2.59. What is K, for the weak acid?

A: pH = 2.59 pH = -log [H+]2.59 = -log [H+] [H+] = 10-2.59   Relationship between the dissociation…

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: Calculate the hydroxide ion concentration, [OH−], for a solution with a pH of 10.32   [OH^-]= ? M

A: PH is defined as negative logarithm of concentration of [H+] ions.  PH + POH = 14  Given , PH =…

Q: a sample of freshly pressed apple juice has a pOH of 11.11. Calculate [H+]

A: There is relation between POH , pH , [OH-] , [H3O+] # POH + pH = 14 # [H+] = 10 - pH  by using this,…

Q: Complete the table below: Calculate the values of both the pH and the pOH of the following solutions…

A:

Q: Calculate the pH and pOH of each of the following solutions. a. [H*] = 1.0×10¬M b. [H-] = 7.9x10--M…

A: a) [H+] = 1.0×10-4 M We know that,     pH   = -log[H+]             = -log(1.0×10-4 M)             =…

Q: The pOH of a basic solution is 2.75. What is pH?

A:

Q: at 25 degrees C,  a solution has a hydronium ion concentration of 1.20*10^-9M. What is the pH, pOH,…

A:

Q: The pOH of a basic solution is 5.85. What is [OH⁻]?

A:

Q: What is the pH of a 1.31E-2 molar H 30 * solution? ( pH = log[H1)

A:

Q: Calculate the pH and pOH of each of the following solutions at 25 °C for which the substances…

A: [HCl] = 0.200 M [NaOH] = 0.0143 M

Q: Identify the conjugate acid of So in the reaction below? sơ, (aq) + HSO;(aq) = H SO;(aq) + SO (aq)…

A: Given: HSO4- +SO32- <----> HSO3- +SO42-

Q: Весause s is a strong acid, it dissociates almost com- pletely in water. That means the…

A: We have given that, the concentration of H+ is nearly equal to the concentration of HNO3.

Q: Calculate both the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide…

A:

Q: If the pOH for a solution is 3.00, what is the pH

A: POH = 3.00 PH = ?

Q: Which of the following is the most acidic (lowest PH) pOH of 2.0 [OH-] = 1 x 10-7 m [H+]=4.6 x…

A: Given solutions: pOH of 2.0 [OH-] = 1 x 10-7 M [H+]=4.6 x 10-6 M [OH-] = 1 x10 -8 M pH of 9.5 We…

Q: What is the pH of a 0.0245 M HCl solution?

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Calculate the pH and pOH for each of the solutions with the following hydrogen ion or hydroxide ion…

A: The equations which we relate pH and pOH are  pH + pOH = 14 And the pH and pOH of any solution is…

Q: The pOH of a basic solution is 5.63. What is [OH⁻]?

A: POH is defined as, POH = – log [OH–]

Q: Calculate the pH and the pOH of each of the following solutions at 25 °C for which the substances…

A: The negative logarithm of hydrogen ion is called pH of a solution. The negative logarithm of…

Q: Calculate the pH and the pOH of each of the following solutions at 25 °C for which the substances…

A: Given solutions, (a) 0.000259 M HClO4(b) 0.21 M NaOH(c) 0.000071 M Ba(OH)2(d) 2.5 M KOH

Q: The hydroxide ion concentration of a solution is 7.5 x 10–4 M (7.5e-4). What are the pOH, pH, and…

A: The pH is the concentration of H+ ion in the solution. It can tell us if the solution is acidic or…

Q: The pOH of an acidic solution is 10.15. What is [OH⁻]?

A: pOH of any solution is given by  pOH = -log[OH- ] where [OH- ] = concentration of OH- ions in the…

Q: The pOH of a basic solution is 2.81. What is pH?   The pOH of an acidic solution is 11.55. What is…

A:

Q: An aqueous solution is found to have an OH- concentration ( [OH-] ) of 1.0 x 10-8 M, a) What is the…

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: The pH of a 0.220M solution of a weak acid, HB, is 2.51. What is Ka for the weak acid?

A: Given  PH of weak acid = 2.51  Concentration of weak acid ( c ) = 0.220 M  Ionization constant ( Ka…

Q: The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? 4.2 x…

A: Given that, pH =4.80 Then, [OH-] = ?

Q: The pH of ammonia, a cleaning product used in homes, is 11.61.  What is [OH-]? (0.004 M)

A: To calculate the pH of an aqueous solution you need to know the concentration of the Hydrogen ion in…

Q: What is the pH of a 5.737E-12 molar OH solution? (pOH = -log[OH ]and pH + pOH = 14) %3D

A: pH of a solution is used to identify whether the solution is acidic or basic in nature. The pH of…

Q: 4. The OH- ion concentration of a blood sample is 2.5 x 10-7 M. What is the pH of the blood? pOH…

A: In this question, we have to first find out the pOH of the blood then, we can find pH from it.

Q: NH3(aq) + H₂O(1) = NH(aq) + OH- (aq) The equilibrium hydroxide concentration in a 0.0220 M NH3…

A: Concept based on the pH calculation of the the given concentrated solution.

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

A:

Q: The concentration of a strong monoprotic acid is 0.0010 M.  What is the [OH-]? What is the pH?

A: We calculate the pH of an acid or base using the Sorenson pH scale.…

Q: When a 3 L solution is prepared by dissolving 1,89 g of HNO3 in water, what are [H +], [OH-], pH and…

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.