With detailed explanations, calculate the PH of a solution made by mixing equal volumes of 0.01M butanoic acid and 0.1M sodium butanoate. What type of solution could this be?

Q: What is the pH of a solution prepared by mixing 25.0 mL of 0.180 M HC,H30, with 40.0 mL of 0.250 M…

A: pH of the solution = 13.71

Q: You are given three unknown solutions. One is strongly acidic (pH below 1), one is neutral, and one…

A: pH indicators are added in small amount to solutions so that they can indicate their pH by showing…

Q: Calculate the pH of a mixture of 106 mL of 0.112 M HI and 30 mL  of 0.45 M KOH

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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 a solution made by mixing 100.0 mL of 0.110 M NaBrO with 75.0 mL of 0.140 M…

A: Given: Concentration of NaBrO = 0.110 M Concentration of HBrO = 0.140 M Volume of NaBrO = 100.0 mL…

Q: Calculate the pH of the resulting solution when 350.0 mL of .400 M HCl is mixed with 35.0 mL of…

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Q: Calculate the pH when 68.0 mL of 0.250 M HCl is mixed with 40.0 mL of 0.150 M Ca(OH),.

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Q: Calculate the pH of a solution obtained by mixing 500.0 mL of 0.10 M NH3with 200.0 mL of 0.15 M HCl.

A: NH3 is a weak base and HCl is a strong acid. When they are mixed, the following reaction takes…

Q: A solution is prepared by mixing 585 mL of 0.600 M NH3 and 320 mL of 0.600 M HCI. Assuming that the…

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Q: What is the pH of the solution obtained by mixing 35.00 mL of 0.250 M HCI and 35.00 mL of 0.125 M…

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Q: What should the pH be for a 0.1 M solution of a strong monoprotic acid? If these strong acids are at…

A: pH calculation for a strong monoprotic acid :

Q: The PH of 0.10 M methylamine is 11.8.when chloride salt of methylamine is added to this solution…

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Q: Calculate the pH when 15.52 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: The neutralization reaction is given below.

Q: What is the resultant pH after mixing 30.0 mL of 0.50 M HCI with 20.0 mL of 0.90 M NaOH? Express…

A: Given: Concentration of HCl = 0.50 M Concentration of NaOH = 0.90 M Volume of NaOH solution = 20.0…

Q: Calculate the pH of the solution that results from mixing 20.0 mL of 0.0500 M HCN solution with 80.0…

A: The given solution contains: 20.0 mL of 0.0500 M HCN and 80.0 mL of 0.030 M NaCN solution.

Q: Calculate the pH of a solution made by mixing 25.00ml. of 0.1056M HCI with 13.23ml of 0.1138M NAOH…

A: The acid solution is the solution in which loss of proton takes place and the pH of the solution is…

Q: Calculate the pH of a solution prepared by mixing 45.0 mL of 1.45 M sodium hydroxide with 56.0 mL of…

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Q: How many milliliters of acetic acid with a concentration of 10M should be added to a liter of 0.09M…

A: Value of pH is used to calculate acidity or basicity of a solution. pH value of a solution at room…

Q: Calculate the pH when 19.15 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: The neutralization reaction is given below.

Q: Calculate the pH of a solution prepared by mixing 0.080 0 mol of chloroacetic acid plus 0.040 0 mol…

A: The molarity of chloroaccetic acid and sodium chloroacetate solutions are first determined as shown…

Q: Calculate the pH of a mixture containing 0.266 mol HBz and 0.124 mol NaBz dissolved to 500.0 mL with…

A: Answer:- This question is answered by using the simple concept of calculation of pH of the solution…

Q: Calculate the pH of a solution obtained by mixing 25.00 mL of 0.20 M NH3 with 25.00 mL of 5.0 x 10-2…

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Q: Calculate the pH of a solution obtained by mixing 449 mL of0.17 M nitric acid with 405 mL of 3.6 x…

A: Since both the acid and base are strong in nature  Hence they will react until one of them gets…

Q: Calculate the pH of a solution prepared by mixing 10.0 mL of 0.3 M HCl with 15.0 mL of 0.5 M NaOH.

A: We have given that Concentration of HCl = M1 = 0.3 M Volume of HCl = V1 = 10 mL Concentration of…

Q: A mixture is made by combining 110 mL of 0.015 M HCl and 215 mL of 0.025 M HI. What is the pH…

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Q: Calculate the pH when 9.06 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: From the molar equation-   M1: molarity of NaOH solution. V1: volume of NaOH solution. M2: molarity…

Q: Calculate the pH when 4.91 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: The volume of NaOH solution is 4.91 mL which is equal to 0.00491 L and the volume of acetic acid is…

Q: A solution is prepared by mixing 25 mL of 0.06 M NaOH with 65 mL of 0.125 KOH. What is the pH of…

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Q: Which acid would be the best to combine with its sodium salt to make a solution buffered at pH 5.25?…

A: Here we have to determine the mass of sodium salt of conjugate base required to form buffer solution…

Q: Calculate the pH of a solution prepared by mixing 15.0 mL of 0.10 M NAOH and 30.0 mL of 0.1 acid…

A: Determination of no. of mol of NaOH: n=M×V=0.10 mol/L×15.0×10-3L=1.5×10-3 mol Determination of no.…

Q: Calculate the pH of a solution prepared by mixing 50ml HCl 0.15 with 100ml NaOH 0.05M

A: HCl is a strong acid and NaOH is a strong base. They react together according to the equation: HCl +…

Q: Calculate the pH of a solution formed by mixing 100.0 mL of 0.100 M NaF and 100.0 mL of 0.025 M HCl

A: Answer:- This question is answered by using the simple concept of calculation of ph of a solution…

Q: Calculate the pH after 75.0 mL of 0.100 mol L- HCl solution has been added to 100.0 mL of 0.100 mol…

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Q: Calculate the pH when 5.48 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

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Q: What is the pH of a solution prepared by mixing 45.0mL of 0.183 M KOH and 65.0mL of 0.145 M HCL?

A: Moles of HCl = 65 x 10-3 L X 0.145 = 0.009425 mol Moles of KOH = 45 x 10-3 X 0.183 = 0.008235 mol

Q: Calculate the pH obtained by dissolving 2.5 g of KoH in a solution containing 0.01M HCl in a volume…

A: Given Values: Weight of KOH dissolved in 100 ml of 0.01 M HCl solution = 2.5 gram Molecular weight…

Q: An aqueous solution contains 0.485 M acetic acid. Calculate the pH of the solution after the…

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Q: Calculate the pH of a solution containing 200ml of 0.01M NaOH and 8ml of 0.25M of acetic acid.

A: Answer :-  The pH of a solution containing 200ml of 0.01M NaOH and 8ml of 0.25M of acetic acid =…

Q: Calculate the pH of a solution obtained by mixing 500.0 mL of 0.10 M NH3 with 200.0 mL of 0.15 M…

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Q: What volume (in mL) of a 1.0 M solution of imidazolium chloride must be added to a 500 mL solution…

A: Buffer solutions are the solutions which counter the pH change on addition of small amount of acid…

Q: A 1.0 M solution of hydrochloric acid is mixed with an equal volume of sodium hydroxide solution.…

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Q: The pH of 0.10M methylamine is 11.8. When the chloride salt of methylamine is added to this solution…

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Q: If 1.0 mL of 0.4 M HCl was added to 40.0 mL of pure water, what would the resulting ΔpH of the…

A: Since moles of HCl taken = volume of HCl in L X molarity of HCl = 0.4 X 1 / 1000 = 0.0004 Since HCl…

Q: Calculate the pH change by taking 40 mL of 0.1M HCl with adding a 0.1M NaOH of 50 mL of the base

A: Given Values: Initial solution= 0.1 M HCl with a volume of 40 ml Now, 50 ml of 0.1 M NaOH is added…

Q: What is the pH of the solution obtained by mixing 35.00 mL of 0.250 M HCl and 35.00 mL of 0.125 M…

A: Given, Volume of HCl = 35.00 ml Volume of NaOH = 35.00 ml Molarity of HCl = 0.250 M Molarity of NaOH…

Q: calculate the pH of a solution prepared by mixing 456mL of 0.10M HCl with 285 mL of 0.15M NaOH.

A: The pH depends on -log of concentraion of H+ ion present in the solution.so first of all we have to…

Q: Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The…

A: The indicator that used to determine the pH of solution more precisely, has to be given.

Q: what is the pH of 100ml of the solution containing 0.01-mole acetic acid and 0.01-mole sodium…

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Q: A solution is prepared that is initially 0.069M in ethylamine (C,H,NH,), a weak base, and 0.15M in…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.