The pH is dependent on which of the following? acid concentration Owhether the acid is strong or weak Oboth choice a and b Oneither choice a nor b

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

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Q: 48) Which of the following is a weak acid? A) HCI B) HBr C) HF D) H,SO, E) NaOH

A: Strong acid- an acid dissociate immediately into its ions in an aqueous solution to give H+ ions.…

Q: each of the following as a strong acid or a weak acid and indicate how each should be written in…

A: The main difference between a strong acid and weak acid is that strong acids are 100 % ionizable in…

Q: Which of the following statements describes a 0.010 molar weak acid solution? a) not enough…

A: pH of a solution is defined as the negetive logarithm of concentration of H+ ion.  Here the…

Q: Calculate the pH of the following solution: 1.0 M H

A: pH = -log [H^+] Given -> [H^+]=1.0M

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

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

Q: write the eacion for the acidic and basic Salts mchen It is dissolived m waier. write The met ionic…

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Q: Calculate the pH a 0.060 M HF sulution?

A: Given  [HF] = 0.060 M Ka of HF = 6.6 x 10-4 The dissociation reaction of HF can be written as -…

Q: Assuming equal concentrations, arrange these solutions by pH. Highest pH

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

Q: the pOH a basic solution is 3.55 what is [H+]

A: Given: pOH of basic solution = 3.55

Q: Calculate the pH and pOH of A) 0.0010 M NaOH B) 0.125 M HCl

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Q: If the ?aKa of a monoprotic weak acid is 7.9×10−6,7.9×10−6, what is the pH of a 0.25 M0.25 M…

A: The question is based on the concept of equilibrium. we have been given a weak acid whose…

Q: If the ?bKb of a weak base is 1.5×10−6,1.5×10−6, what is the pH of a 0.34 M0.34 M solution of this…

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Q: Solution A has a pH of 5.6. Solution B has a pH of 2.8. Which has a higher (H*] concentration? O…

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Q: A solution has a pOH of 13.12. This tells us   a) solution is very acidic b) solution is slightly…

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Q: How can a weak acid solution have the same pH as a strong acid solution?

A: pH = -log [H^+] Hence, pH depends on H^+ concentration.

Q: The conjugate base of a weak acid is   Question 3 options:   A)  a strong base.    B)  a strong…

A: The conjugate base of weak acid depends on the stability of the conjugate base.

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

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Q: What is the pH and pOH of a: a) 0.20M NH4CI solution? b) 0.47M NaCN solution?

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Q: CsBr neutral, basic, acidic, or cannot be determined?

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Q: What is the Ka if the pH of the half-neutralized solution is 1.86?

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Q: Calculate the pH of each of the following solution? a) 0.10 M HCl b) 0.10 M NaOH

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Q: What mass (in grams), of KOH is needed to prepare a 1.750L solution having a pH of 12

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Q: Sorbic acid, is widely used in the food industry as a preservative.  For example, its potassium salt…

A: Interpretation: Sorbic acid, is widely used in the food industry as a preservative. for example, its…

Q: H0

A: Acid: The substance which donates H+ ion in the aqueous solution is known as an acid.

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: Calculate the pH of each of the following solutions of strong acids A) 1.34e-3 M  HNO3 B) 0.000187…

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

Q: nobasic acids. pH value than CH,SO,OH with

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

Q: Aspirin, which is acetylsalicylic acid, was the first NSAID use to alleviate pain and fever. If a…

A: Since the concentration of H+ ions is always ( in any case) = concentration of H3O+  hence [H+] =…

Q: 57.0 ml of 0.90 M solution of HCl was diluted by water. The pH of this diluted solution is 0.90. How…

A: Dilution :-  If a solution of molarity M1 and volume V1 is diluted by adding water to a solution of…

Q: Identify the weak acid from the list. - HF - H2CO3 - H2SO2 - all of these

A: The species that increase the concentration of hydrogen ions or hydronium in an aqueous solution act…

Q: Would the pH of a solution of a base be higher than, lower than or the same as the pH of a solution…

A: The pH scale is a logarithmic scale that measures the acidity or alkalinity of a solution. It ranges…

Q: What is the pH of a strong, monoprotic acid solution with a concentration of 0.763M?

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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.