Calculate the pH of the following solution at 25 °C for which the substance ionizes completely: 0.259 M HCl

Q: 69. A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant…

A: A weak acid are those which does not completely dissociate to liberate H+ ion

Q: The hydronium ion concentration in an aqueous solution at 25°C is 1.1×10-3 M. The hydroxide ion…

A:

Q: Calculate the pH that results when the following solutions are mixed: 35 mL of 0.20 formic acid, 55…

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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: The hydroxide ion concentration in an aqueous solution at 25°C is 1.1×10-2 M. M. The hydronium ion…

A: The pH of a substance can be expressed as the negative log of the hydrogen ion concentration. It is…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 8.3×10-2 M. The hydroxide ion…

A: The pH is a method that helps in determining whether the given solution is acidic or basic. Given…

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the pOH of the solution. Is the…

A:

Q: Calculate the pH and pOH of 0.01 M ammonium hydroxide ( NH.OH ) , if the Percent ionization of NH OH…

A: We know that  [OH-]= C×degree of dissociation C=0.01 Degree of Dissociation=0.00125…

Q: solution

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Calculate the pH of an aqueous solution of 0.1340 M potassium sulfite. pH = ||

A:

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 an aqueous solution that contains 8.5x10-2 M hydroxide ion

A:

Q: The pH of an aqueous solution of 0.393 M nitrous acid is

A:

Q: The pH of an aqueous solution of 0.512 M nitrous acid is

A: Given 0.512M Nitrous acid HNO2 Pka of Nitrous acid  [H+] = (7.2*10-4*0.512)1/2 [H+] = 0.0192

Q: The hydronium ion concentration in an aqueous solution at 25°C is 1.4×10-4 M. The hydroxide ion…

A: The formula that will be used : pH = -log(H3O+)  pOH = -log(OH-)  pH + pOH = 14 Given, H3O+ = 1.4 x…

Q: Calculate the pH and the pOH of an aqueous solution that is 0.0500.050 M in HCl(aq)HCl(aq) and…

A:

Q: Determine the pH for the following salts in water. Assume that you have a 0.20M solutions of each of…

A: As you have posted multiple subparts in 1 question. Hence we are solving only the first 3 subparts…

Q: Calculate the pH of each of the following solutions of strong acids.

A:

Q: For the reaction of C5H5N with water, write the base ionization constant expression.

A: we have to write the expression for  base ionization constant for reaction of C5H5N with water

Q: Determine the pH of a solution that is 0.20 M in NH3 and 0.30 M NH4Cl

A: The mixture of NH3 with NH4Cl is a buffer solution as it is a mixture of weak base (NH3) with its…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 9.7×10-2 M. The hydronium ion…

A: Given, Hydroxide ion concentration [OH-] = 9.7 X 10-2 M T = 250 C So we've given the concentration…

Q: Calculate the pH AND the pOH of each of the following solutions 9) 150,000 mL of a solution…

A:

Q: Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCI(aq) and 0.060 M in…

A: Answer :-  1) 0.030 M HCl    a) pH = 1.52     b) pOH = 12.48…

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: Calculate the pH of the solution after the addition of 2.91×10o-² moles of sodium hydroxide to 255…

A: Given: Concentrationof acetic acid = 0.340M Volume of NaOH = 255ml = 0.255L Number of moles of NaOH…

Q: pH of an aqueous solution of 0.355 M acetylsalicylic acid (aspirin) , HC9H7O4, is .

A:

Q: Consider a solution which is [OH-] = 8.4 x 10-11 M. Calculate the pOH of the solution. Is the…

A: [OH–] = 8.4 x 10–11 M( Given ) So, pOH = – log [OH–]  = – log( 8.4 x 10–11 ) = 10.075 Now, As we…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 5.3x10-3 M. The hydroxide ion…

A: PH = - log[H3O+] Ionic product of water : [H3O+] [OH-] = 1 x 10-14 POH = - log[OH-]

Q: The pH of an aqueous solution of 0.236 M sodium cyanide, NaCN (aq), is This solution is acidic,…

A: NaCN is salt of strong base and and weak acid. The chemical nature of the solution depends on the…

Q: The pOH of an aqueous solution at 25°C was found to be 3.90. The pH of this solution is The…

A: Using the relation between pH and pOH and formula of pH we can solve given parts.

Q: A solution contains 0.378 M potassium acetate and 0.374 M acetic acid. The pH of this solution is…

A: Acidic buffer solution :- A mixture of weak acid and salt of weak acid with strong base is called…

Q: Determine the pH of the following: 1.00 × 10–6 M KOCl solution

A: We have to determine the pH of the following: 1.00 × 10–6 M KOCl solution

Q: The pH of an aqueous solution of 0.124 M ammonium nitrate, NH4NO3 (aq), is ___________. This…

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: Calculate the pH of an aqueous solution of 0.2100 M potassium carbonate. pH

A:

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

A: POH = 3.00 PH = ?

Q: Complete each of the following equations. Then write the Lewis formulas of the reactants and…

A: Lewis gave the definition of an acid or base. According to him, an acid is a substance which can…

Q: Calculate the concentration of H + in a solution of silicic acid of 1 mol / liter. Calculate the pH…

A: Concentration of silicic acid = 1 mol/L Concentration of H+ = ?  pH of the solution = ?

Q: Calculate the pH of an aqueous solution of 0.141 M potassium sulfite. pH = .

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 1.7×10-2 M. The hydronium ion…

A: pH of any solution decided it is of acidic in nature or basic in nature or it is neutral.

Q: 1.21 х 103 М HNO3

A: Calculate the pH of each of the following solutions of strong acids.

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: What will be the pH value of the solution if we have added aqueous NH4Cl to a neutral solution and…

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 0.46 MRbOH(aq)  solution

A:

Q: Determine the pH of a 0.100 M solution of butanoic acid, whose percent deprotonation (aka percent…

A: The dissociation of butanoic acid is as follows: CH3CH2CH2COOH <--------->CH3CH2CH2COO-(aq) +…

Q: If a sample of a certain solution is determined to have a [H3O^+] concentration of 4.89×10^−1…

A: Given: [H3O+ ] = 4.89 × 10-1 M.

Q: Calculate the pH of an aqueous solution of 0.1930 M sodium carbonate. pH =

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 2.2×10² M. The hydronium ion…

A: given dataOH-=2.2×10-2M

Q: Calculate the pH and the pOH of an aqueous solution that is 0.045 M in HCI(aq) and 0.055 M in…

A: pH = -log[H+] pH + pOH = 14 [H+] = [HCl]  [H+] = [HBr]

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.