The pH of the solution formed by mixing 25 ml of 0.1 M KOH solution with 24.9 ml of 0.1 M HNO3 solution is: a) 10.3 b) 3.7 c) 7 d) 13

Q: Calculate the pH of(a) a solution that is 0.250 M in sodium formate (HCOONa)and 0.100 M in formic…

A: (a). Given information; The initial concentration of formic acid (HCOOH) is 0.100 M The initial…

Q: Calculate the pH of a solution that is 0.1230.123 M HClHCl

A: To calculate pH of a solution:

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH  = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: Calculate the pH of a mixture that contains 0.23 M of HCNO and 0.16 M of HBrO. The ?a of HCNO is…

A: Given: Concentration of HCNO=0.23 MConcentration of HBrO=0.16 MKa of HCNO=3.5×10-4  Ka of…

Q: ate the pH of a hydrobromic acid solution prepared by a for a final volume of 750mL. a. 3.36 b. 2.42…

A: The chemical formula of hydrobromic acid is HBr. It is a strong acid. When it is dissolved in water,…

Q: Calculate the pH of a solution that is 9.00 % (w/w) NaOH and has a density of 1.098 g mL-1.

A: To calculate the pH of the given solution, first of all, we calculate the concentration of hydroxide…

Q: Calculate the pH of each of the following strong acid solution 5.00 mL of 0.250 M HClO4 diluted to…

A: The process applicable for lowering the particular stock solution's concentration gets addressed as…

Q: Consider a HCl solution that has a pH of 4.70. a) Calculate the concentration of HCl.  b) Identify…

A:

Q: The pH of a solution of household ammonia, a 0.950 M solution of NH3, is 11.612. Determine Kb for…

A: We know that, pH can be expressed as the negative logarithm of H+, i.e.            pH = - log[H+]…

Q: Q3// Grams of Sodium Formate required to add to 400ml of o.1M Formic acid to make the pH of solution…

A: The given solution is a buffer of Formic acid and Sodium formate. The pH of a buffer solution is…

Q: if 65ml of 0.25M naoh are combined with 76ml of 0.3M h2so4 .What is the pH if the solution is…

A: Given  Millimoles of H2SO4 = M x V = 0.3 x 76  = 22.8 mmol Millimoles of H+ ion = 2 x millimoles of…

Q: The pH of a solution prepared by mixing 50.0 mL of 0.125 M NaOH and 30.0 mL of 0.125 M HNO3 is…

A:

Q: A solution is made by dissolving 22.3 g of HONH₃ClO₃ in 500.0 mL of water. Using Ka(HONH₃⁺) = 9.1 ×…

A: OHNH3ClO3 dissociates to give H+ ions in the solution. The net ionic equation is:

Q: What

A: We will use concept of pH of salt

Q: The pH of a solution of household ammonia, a 0.950-M solution of NH3, is 11.612. What is Kb for NH3.

A:

Q: 10

A: NaCN is a salt of strong base and weak acid. The pKa of HCN can be calculated as follows-

Q: If the Kb of a weak base is 6.8*10^-6 what is the pH of 0.18M solution of this base

A: We have to calculate the pH of weak base.

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0104 M solution. The pH of the…

A: Given: Concentration of weak acid solution is 0.0104 M. pH of the weak acid solution is 2.48.

Q: The graph given below shows [H+] versus concentration foran aqueous solution of an unknown…

A: a) Since the concentration of H+ i.e [H+] is increasing with increase in the concentration of…

Q: Consider a HCI solution with a pH of 4.70. a) Calculate the concentration of HCl. b) Identify the…

A: pH is he negative logarithm of hydrogen ions. pH values can range from 0 to 14. pH is used to know…

Q: Suppose that a benzoic acid (C,H,COOH) solution has a pH of 3.15. Which of these substances would…

A: Given substances: KCl C6H5COONa NaI HBr We have to find the substance that would increase the pH…

Q: The pKa of HOCl is 7.5. Calculate the pH of a 0.31 M solution of HOCl. How else can this concept be…

A: pKa: It is used to indicate strength of an acid. And it is obtained by negative log of acid…

Q: A 0.020 M solution of niacin has a pH of 3.26. Calculate the percent ionization of the niacin.

A: Given information: pH = 3.26 Concentration of acid = 0.020 M

Q: What is the pH of a solution that has a hydrogen ion con- centration of 1.0 X 10 M? 46. TATI

A:

Q: What mass of HNO, is present in 211.0 mL of a nitric acid solution having a pH = 5.70? 5.96e-5

A: Given data :  pH of solution = 5.70  Volume of Solution = 211.0 ml = 0.211 L

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

A:

Q: What is the pH of a solution containing 0.25 M HCOOH and 0.51 M HCOOK?

A:

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.77 M solution. The pH of the…

A: Given: Concentration of monoprotic acid = 1.77 M pH of solution = 2.72

Q: 6. Calculate the pH of the following solutions at 25 °C: a. 0.25 M KOH b. 0.75 M NH4I C. a solution…

A: as mentioned, we are solving question 6 (a-d) for you

Q: 0.020 M solution of niacin has a pH of 3.26. Calculate the percent ionisation of the niacin.

A: To calculate the precent ionisation of the niacin we first calculate the [H+] pH = 3.26  [H+] =…

Q: 2.30 mL ofa 0.4375 M HCl solution are added to 35 mL of 0.250 NAOH solution. What is the final pH?

A: An acid HCl and base NaOH undergo neutralization reaction to form salt NaCl and water. For the given…

Q: An aqueous solution at 25 °C is 10.4% HNO, by mass and has a density of 1.054 g/mL. What is the pH…

A:

Q: How many moles of H₃O⁺ or OH⁻ must you add per liter of HA solution to adjust its pH from 9.33 to…

A:

Q: Enough of a monoprotic acid is dissolved in water to produce a 0.0162 M solution. The pH of the…

A: Given,  The concentration of monoprotic acid = 0.0162 M.  The pH of the solution = 2.57. The Ka of…

Q: 9) What mass of HNO, is needed to make 315.0 mL of a solution with a pH of 2.27?

A:

Q: 2. 30 mL of a 0.4375 M HCI solution are added to 35 mL of 0.250 NAOH solution. What is the final pH?

A: Given: The volume of HCl = 30 mL The concentration of HCl = 0.4375 M The volume of NaOH = 35 mL The…

Q: 4. 4.00 g KOH was added to the less basic solution in number 3. What will be the resulting pH of the…

A: Given, Mass of NaOH = 5.00 g  Mass of Ba(OH)2 = 5.00 g  Gram molar mass of NaOH = 40 g/mol  Gram…

Q: B. Calculate the pH after 17.50 mL of NaOH is added to 35.00 mL of acetic acid using the…

A: pH of a solution is the negative logarithm of the concentration of H+ ions present in that solution.…

Q: The pH of a basic solution is 12.39. What is [H*]?

A: The question is based on pH determination of a solution pH is defined as negative logarithmic of…

Q: When 10 mL of 0.1 M NaOH is added to 50 mL of 0.05 M HCl solution, which of the following is the…

A:

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0199 M solution. The pH of the…

A: In this question, we want to determine the Ka value of weak monoprotic acid.  How we can calculate,…

Q: 7

A: The salt given is NH4C3H5O2.

Q: Calculate the pH of a 1L aqueous solution that is 0.13 M in NH3 and 0.26 M in NH4NO3 after 0.013 mol…

A:

Q: The pH of an aqueous solution at 25.0 °C is 12.36. What is the molarity of H + in this solution?

A: Given information,      The pH of an aqueous solution at 25.0 °C is 12.36

Q: A solution having a pH of 7.85 is:

A: If pH<7 then solution is acidic in nature pH =7  then solution is neutral pH>7 the solution is…

Q: A weak base has a Kb of 4.29E-10. Calculate the pH of a 0.250M solution of the weak base.

A:

Q: Calculate the concentration of HCI in an aqueous HCI solution with a pH of 2.21.

A:

Q: volume

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.