Calculate the pH of the following solution: 1.0 M KOH

Q: Calculate the pH of the following solution: 50 M HNO3

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Q: Calculate the pH of a 0.165 M  solution of KOH.   Calculate the pOH of a 0.165 M  solution of KOH.

A: Concentration of solution of KOH = 0.165 M

Q: 6. Determine the pH and [OH] of a solution if its [H*] = 7.5 x 103M.

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

Q: Calculate the pH of a solution with a hydrogen ion concentration of 4.5×10^-6 M.

A: Given that, in a solution, the hydrogen ion concentration is [H+] = 4.5×10-6 M. We have to calculate…

Q: Calculate the pOH of a solution that is 0.428 M NaOH

A: We know that ,  PH = - log [H+]  POH = - log [OH-]  PH + POH = 14

Q: Calculate the pH of 0.010 M Trisodium arsenate

A: The pH is calculated below

Q: Determine the pH of the following solutions, using the information provided. 1.25 ×10–3 M HNO3…

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Q: Calculate the pH of a 5.714 M solution of NaHS

A: Given Concentration of NaHS is 5.714 M To find pH of the given solution

Q: Calculate the pH of an aqueous solution that is 0.70 M sodium hypochlorite.

A: The given compound Sodium hypochlorite (NaClO) is a strong electrolyte. So, it dissociates…

Q: A solution of sulfuric acid (H2SO4) has a concentration of 0.0075 M. Calculate the pH of this…

A: Given, Concentration of H2SO4 solution = [H2SO4] =  0.0075 M pH of the solution = ? Note:  Sulfuric…

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

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Q: Calculate the pH of a 0.020 M solution of oxalic acid

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Q: Determine the pH in a 0.235 M NaOH solution.

A: pH can be calculated using pOH.

Q: Calculate the pH of solution where [H] = 0.000023

A: pH measure the acidity of the solution.

Q: what is the ph of a solution whose hydrogen ion concentration is 0.015?

A: As we know, HCl is a stong acid. It dissociates completely into H+ and Cl—in a chemical equation –

Q: Calculate the pH for an aqueous solution having a hydrogen ion concentration of 2.15 × 10-3 M.

A: pH = -log[H+] where [H+] = hydrogen ion concentration  Hence substituting the values we get  pH =…

Q: The pH of an aqueous solution of 0.549 M hydrocyar

A: HCN is a weak acid , weak acid does not dissociate completely hence it's pH can be calculated as…

Q: Calculate the pH of a solution that is 0.142 M HCL?

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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: Calculate the pH of a solution that has [H 3O +] = 5.2 × 10 –7 M.

A: pH is the potential of the hydrogen which is usually used to predict how strong an acid is. The pH…

Q: hydrogen

A: You can used the equation,  pH = -log[H+]  Given : [H+] concentration = 1.00 • 10^-4  pH = -log(…

Q: Calculate the concentration of an aqueous solution ofNaOH that has a pH of 11.50.

A: Given: pH of NaOH solution is 11.50

Q: Determine the pH of the following solutions, using the information provided. 3.00 × 10–9 M KOH

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Q: Calculate the pH of the following solutions of strong acids: HNO3 0.0575 M

A: Here, we have to calculate the pH of 0.0575 M HNO3 solution.

Q: Calculate the pH of a 0.20 M solution of HCN

A: Given data 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: Calculate the pH of a solution if the concentration of OH- is 6.79 x10^(-8) M

A: Given, [ OH-] = 6.79 *10-8M

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: Calculate the pH of each of the following solutions: (a) 0.0010 M HCl (b) 0.76 M KOH

A: The pH and pOH of the solution can be determine by using the formula is as follows;

Q: Calculate the pH of the following solutions.  - 0.10 M pyridine

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Q: Calculate the pH of the following solutions: a) HCL 0.2 m B) CH3COOH 0.2 m

A: (a) Given data contains, Molarity of HCl is 0.2M.

Q: The hydroxide ion concentration in a dilute ammonia solution is 0.0025M. Calculate the PH of the…

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Q: Calculate the unknown pH of a solution Using the hydrogen lon concentration.. pHi (H,0 1.0 x 10 1.5…

A: The buffer solution is defined as the aqueous solution which consists of a weak base/acid and its…

Q: What is the pH of a solution if the given is -4 [OH¯] = 4.5x10¬ M?

A: Given that: [OH-] = 4.5×10-4 M

Q: The hydronium ion concentration in a given solution is 1.8 x 104. What is the concentration of the…

A: Hydronium ion concentration H+ and hydroxide ion concentration OH- are related to each other as:…

Q: Calculate the pH of a 0.74 M solution of NaOH.

A:

Q: Calculate the pH of a 0.150 M  solution of KOH. Calculate the pOH of a 0.150 M  solution of KOH.

A: We have given that  Calculate the pH of a 0.150 M solution of KOH. Calculate the pOH of a 0.150 M…

Q: Calculate the pH of each of the following strong acid solutions: (a) 8.5 * 10-3M HBr,

A: pH is a measure of how acidic/basic water is. The range goes from 0 to 14, with 7 being neutral. pHs…

Q: 8) Determine the pH of the following solutions: a) 0.20 М СHСООН

A: The answer for part a) is given below. Kindly post the other subpart as separate question

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

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Q: Calculate the hydrogen-ion concentration and pH of 0.0350 M KOH.

A: KOH completely dissociate into  KOH ------>K +  + OH- At 25o C  Ionic product (K w )   of  water…

Q: Calculate the pH of a 0.55 M solution.

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Q: Calculate the pH of solutions with the following concentrations. [OH−]= 1×10−12M

A: Given, [OH-] = 1 * 10-12 M   Required,                      pH of the solution   First, have to find…

Q: Calculate the pH of each solution. H3O+][H3O+] = 6.0×10−7 M

A: pH  calculation using concentration of H+ :

Q: Calculate the pH of a 0.00118 M solution of HBr.

A: Given data contains, Concentration of HBr is 0.00118 M. Hydrobromic acid is a strong acid so it gets…

Q: Calculate the pH and the pOH of the solution at 25 °C.

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Q: Calculate the pH of a 1.77 M NH4CN solution.

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

Q: Calculate the pH of a solution with [H+]= 1×10−4 M .

A: The pH of a solution is calculated by using the hydrogen ion concentration by using the following…

Q: Calculate the pH of the following solutions. 0.40 M phthalic acid

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.