what do you expect to happen to the pH of the same if you add 11 ml of i M NaOH instead of 11 ml of 1 M HCl

Q: What is the change in pH when adding 20.0 mL of 0.150 M NaOH to half a liter of pure water?

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Q: You have 100mL of 0.1M HCI in a beaker and you begin to add NaOH to the beaker. Consider the…

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Q: What is the pH of a solution that is 2.0 M HF and 2.0 M F–?  Does your answer make sense?

A: The Henderson Hasselbalch equation for acidic buffer is given as :

Q: What is the pH of a solution in which 15 mL of 0.39 M NaOH is added to 25 mL of 0.39 M HCl?

A: Since NaOH and HCl are strong base and acid respectively Hence they will react as per the reaction…

Q: Explain why the pH does not change significantly when a small amount of an acid or a base is added…

A: The solution of a weak acid or base with its conjugate base or acid respectively is known as a…

Q: How many ml of 0.5 M HCl must be added to 100.0 ml of a 0.2 M Imidazole (C3H4N2 ; Kb=6.3x10-8)…

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Q: Calculate the pH of a solution that is 1.314 M HF, 0.442 M NaOH, and 0.719 M NaF. For HF K = 7.2 x…

A: Here we have NaOH which is a strong base and will completly dissociate on reacting with HF.

Q: Which solution has the higher pH, a 0.001 M solution of NaOH or a 0.001 Msolution of Ba(OH)2?

A: The simplification is as follows:

Q: Predict the major products of the following organic reaction: D + NC Some important Notes: A ?

A: Given a conjugated diene and dienophile. Draw the major product.

Q: A quantity of 0.15 M hydrochloric acid is added to a solution containing 0.10 moles of sodium…

A: The ratio of the number of moles of a solute dissolved per litre of solution is called the…

Q: 4- A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

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Q: Calculate the pH of the solution that results following addition of 10 mL of 1 M NaOH to 40 mL of 1…

A: Given: The objective is to calculate the pH of the solution  1M NaOH to 40mL of 1M NH4 Cl Formula…

Q: What is the pH of the solution after 50.00 mL of 0.100 M  NaOH  is added to 50.00 mL of 0.100 M…

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Q: A solution is 0.40 M HF and 0.80 M KF. Which of the following actions will result in pH - pK, for…

A: solution which resists it pH by adding small amount strong acid (or) strong base is called buffer…

Q: Explain why the pH does not change significantly when a small amount of an acid or base  is added to…

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

Q: There are 0.2 mole of HC2H3O2 and 0.2 mole of NaC2H3O2 in 0.5 liters of water (pH = 4.75). What…

A: Since no. of moles of acetic acid and sodium acetate are equal, that is 0.2. Thus initially, pH will…

Q: Calculate the pH change that results when 12 mL of 2.1 M HCl is added to 560. mL of each of the…

A: pH change = pH of final solution - pH of initial solution pH = pHfinal - pHinitial

Q: Does the pH of the solution increase, decrease or stay the same when you? (a) add solid ammonium…

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Q: 4- A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

A: The solution of 0.25 M HCOOH and 0.3 M HCOONa is n acidic buffer. Ka of HCOOH=1.75×10-4 We know that…

Q: What is the pH of a solution in which 43 mL of 0.33 M NaOH is added to 13 mL of 0.170 M HCl?

A: Moles of NaOH and HCl are determined as follows,

Q: predicting the qualitative acid-base properties of salts Consid follow name acetic acid acid…

A: An acid is a species which donates Proton while a base accepts proton.     an acid after donating…

Q: M H,SO4. The resulting solution has a pH

A: Applying molarity equation and pH formula MV= M1V1- M2V2  PH = -log (H+)

Q: You are given a 125 mL aqueous solution containing an unknown amount of NH4Cl salt. The solution has…

A: Given that, pH of solution =4.82  volume =125 ml =0.125 L  mass of NH4Cl =?

Q: What is the pH of a solution in which 15 mL of 0.15 M NaOH is added to 25 mL of a 0.10 M HCl ?

A: HCl is a strong acid and NaOH is a strong base. The net ionic equation involved in the titration of…

Q: explain why the ph doesnt change significantly when a small amount of an acid or a base is added to…

A: pH doesn't change significantly when a small amount of an acid or a base is added to a solution that…

Q: a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: a) Calculate the pH after 0.10 mol NaOH is added to 1.00 L of a solution that is 0.6 M HF and 1.00 M…

A: Given: Concentration of HF = 0.6 M Concentration of KF = 1.00 M Volume of solution = 1.00 L Since…

Q: Calculate the pH of the solution that results following addition of 30 mL of 1 M NaOH to 40 mL of 1…

A: M1=1MV1=30mlM2=1MV2=40mlpH=-log[H+][H+]=(M2V2-M1V1)/(V1+V2)

Q: A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

A: First we would Calculate pH of buffer solution using Henderson Hasselbalch equation.  When HCl is…

Q: 4. Twenty milliliters of 0.50 N HOAC is diluted with water to 100 mL, and the resulting solution is…

A:

Q: bund in the human body? e Choose one or more: O HCOO /COO-;Ka = 1.77×10-4 O H3PO4/H2PO42-; Ka =…

A: Buffer solutions that can resist pH change upon addition of acid and base

Q: What is the pH of a mixture consisting of 15.00 mL of 0.160 M HCl and 20.00 mL of 0.120 M NaOH?

A: Volume of HCl = 15.00 ml  ...Or  because 1L = 1000 ml   ...so,  = 15.00 ml × (1L / 1000 ml ) = 0.015…

Q: In industrial environments, benzoic acid, C6H5COOH, is widely used to produce a range of products…

A: Given ,

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.