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

Q: Calculate pH of a solution that is 0.0250M HCl

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Q: calculate the

A: Ammonium chloride (NH4Cl) is salt of weak base-strong type. pKb of weak base = 4.74 Concentration of…

Q: The pOH of an aqueous solution at 25°C was found to be 14.00. The pH of this solution is The…

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Q: Calculate the pH of each of the following strong acid solutions: 1.52 g of HNO3 in 575 mL of…

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Q: The pH of a solution of 0.200 M NaOH is __________.

A: • The values provided in the question are:-     i) Concentration of sodium hydroxide solution,…

Q: Calculate the pH of an aqueous solution; 0.015 M KOH

A: Given: Concentration of KOH = [OH-] =  0.015 M

Q: The pH of an aqueous solution at 25°C was found to be 2.40. The pOH of this solution is The…

A: Given that   Ph of aqueous solution is 2.40

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 and the concentrations of all species in a 0.1500 M NH4NO3 solution.

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Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH−], of 1.35×10−8 M.

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Q: The pH of a basic solution is 10.19. What is [OH⁻]?

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Q: The pH of a basic solution is 10.33. What is [H]?

A: Given details, The pH of the base solution [OH-] = 10.33 To calculate the [H+].

Q: Calculate the pH of an aqueous solution of 0.0740 M potassium sulfite.

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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: Calculate the pH of a  0.500 M HCN solution.

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Q: Calculate the concentration of all species present and the pH of a 0.020-M HF Solution.

A: Concentration of HF = 0.020 MKa(HF) = 3.5 * 10-4Chemical reaction of HF in water Chemical Equation…

Q: Calculate the pH of an aqueous solution of 0.0448 M potassium sulfite.

A: PH is defined as negative logarithms of hydrogen ion concentration.

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

A: pH can be calculated using pOH.

Q: Calculate the theoretical pH for the following solution: . 0.20 M HCl

A: PH= - log [H+]  PH  scale  introduced by Sorensen  Negative logarithm of H + ion concentration known…

Q: The pH of a basic solution is 12.77. What is [H*]?

A: The pH of a solution is mathematically expressed as: pH=-log[H+]   ............... (1) where [H+] is…

Q: The pH of an aqueous solution at 25°C was found to be 6.70. The pOH of this solution is| The…

A: Provided pH=6.70 Concentration of H3O+=10-pH pOH = 14 - pH Concentration of  OH-= 10-pOH

Q: What is the pH of an aqueous solution wit

A: Since you have asked multiparts, we will solve the first three subparts for you. If you want any…

Q: Calculate of pH of a 0.0026 mol/L solution of hydrochloric acid

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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: Enter your answer in the provided box. Calculate the pH of a 0.0825 M HCl solution. pH =

A: HCl completely dissociates since it is strong acid.The concentration of H+ ions for a 0.0825 M HCl…

Q: calculate the Ph of a 0.050M HCl solution

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Q: The pOH of an aqueous solution at 25°C was found to be 7.30. The pH of this solution is The…

A: Given : pOH = 7.30

Q: For an aqueous solution of 0.045 M HNO3, calculate the values of the following parameters:  [H+ ],…

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Q: Calculate the pH of a solutione

A: The pH of a solution, obtained by mixing 449 mL of 0.17 M nitric acid with 405 mL of 3.6 ×10-2 M…

Q: Which one of the following 1.0 M solutions would have the lowest pH?

A: Ph= -log [H+] [H+]= 10-14÷[OH-] Lowest PH=C5H5N  (1) For C5H5NOH- = k6xC = 1.7 x 10-9x1…

Q: Calculate the pH of a 0.27 M sodium carbonate solution. pH= i

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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 an aqueous solution of 0.2100 M potassium carbonate. pH

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Q: Calculate the pH of the following solutions.  0.10 M disodium phthalate

A: Given,  The pH of the solutions. 0.10 M disodium phthalate is:

Q: The pH of an aqueous solution at 25°C was found to be 9.20. The pOH of this solution is The…

A: pH + pOH = 14  pOH = 14 - 9.2 = 4.8

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

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Q: Calculate the pH of an aqueous solution

A: Given :- concentration of sodium sulfite = 0.360 M  concentration of sodium hydrogen sulfite = 0.330…

Q: Enter your answer in the provided box. Calculate the pH of a 0.43 M KOH solution. pH

A: In this question we have to tell the PH of the 0.43M KOH solution.

Q: The hydrogen ion concentration of a basic solution is 9.70 × 10-10 M. What is the pH of the…

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Q: The pH of an aqueous solution at 25°C was found to be 5.40. The pOH of this solution is M. The…

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

Q: Calculate the pH and the percent ionization of a 0.125M HCN solution.

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Q: Calculate the pH of a solution with a hydrogen ion concentration of 0.0003 M

A: Given  concentration of hydrogen ion = 0.0003 M We have to calculate the pH of solution.

Q: calculate the ph of a 0.000427 M barium hydroxide solution.

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Q: Calculate the pH of a 0.150 M solution of KOH. 0.82 Calculate the pOH oíra 0.150M solution of KOH.

A: Given :-  Concentration of KOH solution = 0.150 M  To calculate :-  pH of solution  pOH of solution

Q: Calculate the pH of a solution when3.78grams of HCl was placed in 150.25 mL of water. HCl is a…

A: Solution -

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

A: pH  calculation using concentration of H+ :

Q: Calculate pH of 0.508 M solution of NaOH

A: By using the relation between pH and pOH we can solve this problem.

Q: determine the pH of a 0.0006 M NaOH solution

A: We know that, Negative logarithm of H+ ion is know as pH. pH= -log[H+] & pH + pOH =14 & pOH…

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.