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: if 0.1L of 0.2 HCL is added to 0.9 L of water what is the resultant pH?

A:

Q: he pH of a solution formed by mixing 20.0 mL of 0.250 M formic acid, HCOOH, and 8.0 mL of 0.400 M…

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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: What is the new pH if 0.020 mol HCl had been added to (a) (instead of 0.020 mol NaOH)?

A: As per the given data we have to find the pH after the addition of Hcl which is calculated as…

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: For 280.0 mL of pure water, calculate the initial pH and the final pH after adding 0.024 mol of NaOH

A: pure water : pH = 7.00 moles NaOH = 0.024 [OH-]= 0.024 mol/ 0.280 L=0.0857 M pOH = - log 0.0857=…

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

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

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Q: A 15 ml solution is 0.50 HCI. If 0.2 M NaoH is to added to this solution Calculate the pH of…

A: Given, Volume of HCl solution = 15 mL Concentration of HCl solution = 0.50  Concentration of NaOH…

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: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0178 M solution. The pH of the…

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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: If you are titrating a 20.0 mL of a 0.100 M solution of  HCl with 0.100 M NaOH, what is the pH of…

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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…

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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 solution contains 8.30×10-2 M ammonium bromide and 0.455 M ammonia.The pH of this solution is

A: The objective of this question is to calculate the pH of a solution containing ammonium bromide and…

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: 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…

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

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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: If 55 ml of a 0.50 M solution of HCl is added to 25 mL of a 1.0 M solution of NaOH, calculate the…

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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: How can we calculate the pH of a solution containing either a weak acid or its conjugate base?

A: A buffer solution is formed by the weak acid and its conjugate base of weak base and its conjugate…

Q: Which things should be considered while deciding weak acid/conjugate base pair to make a buffer…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

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 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: Given a buffer composed of HCOOH and NaCOOH (can think of this as COOH-), what happens when a strong…

A: Buffer solution: The buffer solution is an aqueous solution consisting of a mixture of a weak acid…

Q: In the laboratory, a general chemistry student measured the pH of a 0.597 M aqueous solution of…

A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…

Q: If 5.0 mL of 0.40 M NaOH is added to 15.0 mL of 0.40 M HCl, what will be the pH of the resulting…

A: We have given that Concentration of HCl = 0.40 M and Volume = 15 mL = 0.015 LConcentration of NaOH =…

Q: Determine the concentration of a NH,CI aqueous solution that has the pH = 4.0. The base ionization…

A: Given : pH of NH4Cl solution = 4.0  And Kb of NH3 = 1.8 X 10-5  Assuming concentration of NH4Cl…

Q: You add 7.00 mL of 0.100 M NaOH to 50.00 mL of pure water, and to this mixture you then add 12.00 mL…

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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.