Suppose you have just added 100.0 mL of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NAOH. What is the final pH? Enter your answer with two decimal places. The Ka of acetic acid is 1.77 x 105.

Q: What are the Ka values of NH4+ and HF?

A: a)  The Ka Of NH4+ Is 5.6 × 10−10.

Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: The pH of a 0.10 M weak acid solution is determined to be 5.15 at room temperature. Calculate the Ka…

A:

Q: 10 mL of 5.0 X 10 M HCl solution is mixed with 150 mL of water to make a new HCl solution. What is…

A: We have to calculate the pH of solution

Q: The Ka for four acids are H₂CO3: 4.5 x 10-7, HCO₂H: 1.8 × 10-4, H3C,H,O,: 7.1 x 10-4, HCN: 6.2 x…

A:

Q: 6. Determine the pH and [OH] of a solution if its [H*] = 7.5 x 103M.

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: True or false? The pH of a popular soft drink is 2.3; thus the soft drink is basic.

A:

Q: You have a buffer solution containing an acid, HA. The pKa of HA is 7.20 and its conjugate base is…

A: Here we are required to find the pH of the buffer solution.

Q: The formula for the pH of a solution of hydronium ions is given by the logarithmic equation pH=−log​…

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

Q: A chemist dissolves 664. mg of pure nitric acid in enough water to make up 140. mL of solution.…

A:

Q: The pH scale ranges from 0-14. Why do we choose to use this scale to represent hydrogen ion…

A: The hydrogen ion concentration would lies from 1 M to very low value upto 10-14 . So, this is very…

Q: The quality assurance lab just received a shipment of three solutions. The lab manager asks you to…

A: We have to calculate the hydrogen ion concentration of each solution.

Q: What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places. VD…

A:

Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?

A: Given data,pH=2.13Molarity of HA=0.45

Q: A chemist dissolves 670. mg of pure potassium hydroxide in enough water to make up 140. mL of…

A:

Q: A titration of 0.100 M NaOH is titrated into 25.0ml of a 0.100 M HCHO2 solution (Ka = 1.80 x 10 4).…

A:

Q: dont provide handwriting solution..

A: The objective of this question is to calculate the initial molarity of hydrofluoric acid (HF) given…

Q: Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic…

A: The question is based on the concept of pH of the solution.It is defined as a negative logarithm of…

Q: Determine the pH of a solution of a weak acid (HA) that is 0.17 M. The Ka of the weak acid is 7.5 x…

A: Given a concentration of weak acid (HA) =0.17M Acid dissociation constant value =        7.5 x 10-5…

Q: The pH of 0.01 M hydrochloric acid (HCl) is 2, the pH of 0.01 M sulfuric acid (H2SO4) is 1.7, and…

A:

Q: The K, of propanoic acid (C,H,COOH) is 1.34 × 10-³. Calculate the pH of the solution and the…

A: Given : Concentration of propanoic acid i.e HA (assuming HA for ease) = 0.467 M And the Ka of…

Q: A typical aspirin tablet contains 325 mg acetylsalicylic acid. Calculate the pH of a solution that…

A:

Q: A chemist dissolves 849.mg of pure barium hydroxide in enough water to make up 60.mL of solution.…

A: Given,

Q: 1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous…

A: Answer:- This question is answered by using the simple concept of calculation of weak acid and the…

Q: Dindicates concentrat on che pH of a solution, ha

A:

Q: The pH of a 0.70 M solution of propanoic acid (HC,H;0,) is measured to be 2.51. Calculate the acid…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 7. Carbonic acid (H2CO3) is a diprotic acid with Ka1 = 4.30 × 10–7 and   Ka2 = 5.60 × 10–11 What…

A:

Q: The neutralization of an acid with a base yields a salt and usually water in aqueous solution.…

A:

Q: A solution containing 0.0138 M maleic acid and 0.0188 M disodium maleate. The K₁ values for maleic…

A:

Q: Which of the following solutions has the lowest pH?   Group of answer choices   0.3 M Sodium…

A: pH = -log[H+]At a fixed concentration, greater the value of Ka higher is the [H+] and consequently…

Q: Find the pH if the hydrogen ion concentration is 2.8x10-4.

A: Since pH = -log[H+ ]  where [H+ ] = the concentration of the hydrogen ions i.e H+ ions  in the…

Q: The pH of a 0.30 M solution of a weak base B is 10.22. What is the K, of the base? Be sure your…

A:

Q: A solution of sodium cyanide, NaCN, has a pH of 12.00. How many grams of NaCN are in 315 mL of a…

A:

Q: Consider a solution of 1.34×10-3 M hydrochloric acid. What would be the hydrogen ion concentration…

A:

Q: What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M?

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: On a shelf in the lab storeroom marked “Solutions of Acids”, a bottle has a torn label. All that can…

A: Acid dissociates in water to form hydrogen ion and it's conjugate base.

Q: The pH of a 0.16 M solution of a weak acid, HA, is 2.85. What is the value of Ka for the weak acid?

A: The question is based on the dissociation of weak electrolyte. We  have been given a weak Acid which…

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.