For each of the following solutions, calculate the initial pH and the final pH after adding 0.0100 mol of NaOH,

Q: You can find the Ka of a strong acid by running a titration curve.

A: The use of dissociation constant is to measure how well an acid or a base is been dissociated. For…

Q: A solution contains 0.377 M potassium acetate and 8.75×10² M acetic acid. The pH of this solution is

A: Given :-  concentration of potassium acetate = 0.377 M  concentration of acetic acid = 8.75 × 10-2 M…

Q: Calculate the pH of .50M NH3 when .20M NH4Cl is added

A: Given  [ NH3 ]     = 0.50 M  [ NH4Cl ]  = 0.20 M  PH = ?

Q: A student  lab found that a 0.358 M unknown weak acid  is 1.27% ionized. What is the pH value of…

A:

Q: Does the pH and pOH also change after diluting a strong base?

A: Yes, the pH and pOH are changed on diluting a strong base. eg. pH of 1.0 M NaOH aqueous solution =…

Q: the final volume is 1.00 L. Calculate,, and the pH for this solution. [Hint: Concentrated is 38% (by…

A: We are given 49.7mL HCl, 19.1mL nitric acid added in water to make 1 L solution  We have to find pH…

Q: Ka= 1.76 x 10-5 for HC2H3O2 What is the pH of this solution? Table 1 Solution Buffer solution acetic…

A:

Q: For 550.0 mLmL of pure water, calculate the initial pH and the final pH after adding 0.020 molmol of…

A:

Q: A solution contains 0.392 M NH¸I and 0.134 M ammonia. The pH of this solution is

A:

Q: MOH base solution is 0.02 M with an ionization degree of 0.02. The pH of the base solution is

A:

Q: In the laboratory a student measures the percent ionization of a 0.528 M solution of acetic acid to…

A: Consider the given information is as follows; Percent ionization = 0.603% = 0.00603 Concentration of…

Q: The pOH of an aqueous solution at 25°C was found to be 5.90. The pH of this solution is . The…

A: The pH ,hydronium ,hydroxide ion concentration is as follows.

Q: I am having a hard time determining when to use the Hasselbalch equation vs when to use other…

A: Answer: Henderson-Hasslebalch equation is used for the calculation of the pH of buffer solution. To…

Q: 100.0 mL of a 0.109 M HCl solution plus 100.0 mL of a 0.062 M NaOH solution. Determine the pH of…

A: Using stoichiometric ratio we can determine which reactant remains after the reaction. From that we…

Q: Find the pH of the solution when a 50.0 mL of 0.100 M sodium hydroxide is added to 50.0 mL of 0.200…

A: Given,

Q: PRE A Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the…

A:

Q: what the factors involve in a change of the values of a pH initial to a different, final pH?

A: The factors that involve a change in pH from an initial to a final value include:1. Addition of…

Q: How to calculate the ph level of the two solutions mixed? Which is acetic acid and NaOH.

A: The question asks for the method to calculate the pH of a mixture of acetic acid and NaOH

Q: 32.92 mL of 0.24 M NAOH is added to 23.71 mL of a 0.17 M HCI. What is the pH of the solution? Please…

A: Calculate the number of moles of NaOH and HCl. Number of moles = Concentration (M) × Volume…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0184 M solution. The pH of the…

A: Acids are the compounds which donate protons, H+ in the solution. Weak acids partially dissociate…

Q: Calculate the pH after 0.15 mole of NaOH is added to 1.09 L of a solution that is 0.49 M HF and 1.05…

A: The pH after the addition of 0.15 mole of NaOH and 0.30 mole of HCl has to be calculated.

Q: The pOH of an aqueous solution at 25°C was found to be 9.20. The pH of this solution is . The…

A:

Q: At equilibrium, a solution contains 2.0 M ammonia, 1.65 M sodium chloride, 1.25 M potassium…

A: We wil calculate both part of the question.

Q: A 0.15 M solution of a certain weak acid has a pH of 4.00. The K, of the weak acid is

A: Given :-  Concentration of weak acid = 0.15 M  pH of solution = 4.00  To calculate :-  Ka

Q: Find the pH of a solution with a hydroxide ion concentration of 0.025M.

A: hydroxide ion concentration (OH-) = 0.025M.

Q: A 0.316-M aqueous solution of a weak acid has a pH of 2.51. Calculate K, for the acid. K =

A: From given pH value and concentration of solution, ka for acid is found as below

Q: if 50 mL of .5 M NaOH is added with 30 mL of .5 M HCL, what will be the pH of the solution

A: Given :  Volume of NaOH = 50 ml  Concentration of NaOH = 0.5 M  Volume of HCl = 30 ml  Concentration…

Q: A solution contains 0.252 M sodium nitrite and 0.179 M nitrous acid. The pH of this solution is

A:

Q: An aqueous solution contains 0.411 M Na,HPO4 and 0.436 M H,PO4. The pH of this solution is

A:

Q: Find the pH of a solution when 0.01 M HCI and 0.1 M NaOH are mixed in equal * volumes

A: The pH of a solution is defined as the negative logarithm of the concentration of the H+ present in…

Q: Calculate the pH after 10.0 mL of 2.0 M HCI is added to 100.0 mL of 1.0 M pyridine solution, you…

A:

Q: Type your answers in all of Let's consider two dilute acid solutions that are both made at a…

A: pH is the potenz of Hydrogen ion concentration or power of Hydrogen ion concentration. It is the…

Q: 0.1M acetic acid is in a buffered solution with sodium acetate. the ph is 5.50 what is the…

A:

Q: For 480.0 mL of pure water, calculate the initial pH and the final pH after adding 1.5×10−2 molmol…

A: Volume of pure water (H2O) = 480.0 mLAdded HCl = 1.5×10−2 molCalculate the initial pH and final pH

Q: A substance, X is added to a solution, Z. A water molecule is produced. At the end, the pH remained…

A: Given that: The pH of the solution remained constant. When substance X is added, a water molecule is…

Q: A 1.0M HCI solution has a volume of 20.0 mL. Determine the pH of the solution that results from…

A: a) Since the addition of base NaOH will make HCl react with it as per the reaction  HCl + NaOH…

Q: Does pH depend on the concentration of the solution? why?

A: Yes the pH of the solution depends on the concentration of acid in it.

Q: The pOH of an aqueous solution at 25°C was found to be 5.00.The pH of this solution is .The…

A: The objective of this question is to find the pH, hydronium ion concentration, and hydroxide ion…

Q: Calculate the pH of each of the following buffered solutions a. 0.10M acetic acid/0.25M sodium…

A: To solve this question, we will make use of Henderson Hasselbach equation which relates the pH to…

Q: Calculate the pH of the resulting solution if 34.0mL of 0.340 M HCl (aq) is added to 44.0 mL of…

A: Molarity of HCl solution= 0.340 M  Volume of HCl = 34.0 mL Molarity of NaOH solution=0.390 M Volume…

Q: A 0.15 M solution of a certain weak acid has a pH of 4.25. The K, of the weak acid is

A:

Q: A solution contains 0.354 M potassium cyanide and 0.401 M hydrocyanic acid. The pH of this solution…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH = pKa + log SaltAcid…

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.