Calculate the pH of a solution prepared by mixing 20.5 mL of a 0.500 M sodium flouride solution with 32.5 mL of a 0.750 M hydrofluoric acid solution. Use the pKa calculated from question 1.

Q: Suppose a buffer solution contains Z moles of NaOH and 0.025 moles of its salt. The pH of the…

A: Given: Moles of salt = 0.025 mol pH of solution = 9.034 Kb  = 1.8 × 10-5

Q: A solution is made by adding 52.0 mL of 0.230 - M acetic acid (Ka = 1.8 times10^-5) to 52.0 mL of…

A:

Q: Equal quantities of 0.010 M solutions of an acid HA and a base B are mixed. The pH of the resulting…

A: The chemical equation for the reaction between HA and B can be written as follows,

Q: Calculate the pH when 80.0 mL of 0.250 M HCl is mixed with 40.0 mL of 0.150 M Ca(OH)₂.

A:

Q: Find the pH of a solution (adding 0.0100 mol of Ba(OH)2 to 155mL of solution containing 0.0240 mol…

A: Answer:- This question is answered by using the simple concept of calculation pH of solution made by…

Q: A patient is suspected of having low stomach acid, a condition known as hypochloridia. To determine…

A: Milimoles = Molarity × Volume.Number of milimoles of acid is equal to number of milimoles of base in…

Q: Acetic acid (pKa = 4.75) is contained in vinegar. Calculate the pH of the solution prepared by…

A: First to calculate molarity Then to calculate pH using formula.

Q: What is the pH of a solution prepared by mixing 18.00 mL of 0.277M CH3COOH with 50.00 mL of 0.166 M…

A:

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: Solution A is prepared by adding 50 ml of 0.3M hypochlorous acid solution to 50 ml of 0.2M of sodium…

A: Given solution A prepared by mixing of weak acid - hypochlorous acid (HClO) with its salt with…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 42.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: What is the pH of a solution obtained by mixing 0.75 L of 0.147 M  Ba(OH)2 and 0.28 L of 0.0660 M…

A:

Q: A chemist titrates 140.0 mL of a 0.4386 M hydrochloric acid (HCl) solution with 0.3241 M KOH…

A: Step 1:At equivalence moles of HCl and NaOH are equal   Step 2: Step 3: Step 4:

Q: Calculate the pH when 64.0 mL of 0.250 M HCl is mixed with 40.0 mL of 0.150 M Ca(OH)₂.

A:

Q: What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH 3CO 2H with 30.00 mL of 0.030…

A: The question is based on the concept of titrations.   we are titrating  a weak acetic acid with a…

Q: Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: A 9.802-g portion of NaCN was dissolved in enough water to prepare 1.00-L of solution. Calculate (a)…

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is…

Q: what is the pH of a solution prepared by adding 63.6 mL of 0.100 M sodium hydroxide to 69.37 mL of…

A: Given that : The volume of sodium hydroxide = 63.6 mL The molarity of sodium hydroxide = 0.100 M The…

Q: Calculate the pH when 31.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: KOH + HOBr = KOBr + H2O Moles of HBrO = Molarity x volume in…

Q: Calculate the pH in the flask when 50mL of a 0.98 M HI solution have been added to 120. mL of a 0.77…

A: The question is based on the titrations.  we are titrating a strong acid with a strong base. we need…

Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HCIO with 200.0 mL of 0.30 M…

A: Given: Concentration of HClO = 0.20 M Volume of HClO solution = 100.0 mL= 0.100 L…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 21.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁹)

A:

Q: Calculate the pH of a solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl

A: GIVEN:- Calculate the pH of a solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl…

Q: Calculate the pH of a solution made by mixing 200.0 mL of 0.64 M hydrocyanic acid (Ka = 4.9 × 10−10)…

A: Given: The Ka for HCN = 4.9 × 10−10 We have to calculate the pH of a solution made by mixing 200.0…

Q: Calculate the pH when 62.0 mL of 0.250 M HCI is mixed with 40.0 mL of 0.150 M Ca(OH)2.

A: Given that : The volume of HCl = 62.0 mL The molarity of HCl = 0.250 M The volume of Ca(OH)2 = 40.0…

Q: Calculate the pH when 6.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given : concentration of HBrO = 0.3 M and volume of HBrO solution = 20 mL = 0.020 L…

Q: 40.0 mL of a 0.100 mol/L solution of HCL is titrated with 0.100 mol/L solution of NaOH.calculate the…

A: Given : Concentration of HCl = 0.100 M Volume of HCl solution = 40.0 mL = 0.040 L…

Q: Consider the titration of a strong acid, HClO4, with a strong base, KOH. What is the pH of the…

A: Given: 20.0 mL of 0.150 M HClO4  30.0 mL of 0.125 M KOH.

Q: when 100 ml of a .01 M Mg(OH)2 solution is mixed with 100 mL of a .01 M HCl solution, what is the pH…

A: Since both acids and base are strong  hence they will react to form water as shown below Mg(OH)2 + 2…

Q: Calculate the pH of a solution which was made by mixing 50 mL of 0.183 M NaOH and 80 mL of 0.145 M…

A: Welcome to bartleby !

Q: Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given Molarity of KOH = 0.150 M Volume of KOH = 10 ml Molarity of HBrO = 0.300 M Volume of HBrO = 20…

Q: If a buffer solution is 0.180 M in a weak acid (Ka = 1.7 × 10 − 5 ) and 0.600 M in its conjugate…

A:

Q: What is the pH of a solution prepared by mixing 15.0 mL of 0.24 M KOH and 25.0 mL of 0.24 M of…

A: Given data : Concentration of KOH = 0.24 M Volume of KOH = 15.0 mL Concentration of HClO = 0.24 M…

Q: Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given:Concentrations KOH  = 0.150 M    Volume = 50 mLHBrO = 0.300 M   Volume = 20 mLNow number of…

Q: Calculate the pH when 75.0 mL of 0.250 M HCl is mixed with 40.0 mL of 0.150 M Ca(OH)₂

A: According to the question, we need to calculate the pH when 75.0 mL of 0.250 M HCl is mixed with…

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.