Calculate the pH when 25.0 mL of 0.150 M HNO3 is mixed with 40.0 mL of 0.250 M LIOH.

Q: Calculate the pH of a solution that is 0.1230.123 M HClHCl

A: To calculate pH of a solution:

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH  = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: Calculate the pH of:  A solution prepared by combining 25.00 mL of 0.0486 molar sodium cyanide with…

A: Given: Concentration of sodium cyanide (NaCN) = 0.0486 M Volume of NaCN = 25.00 mL Concentration of…

Q: What is the pH of a solution prepared by adding 25.0 mL of 0.10 M HNO3 to 40.0 mL of 0.10 M NH3(aq)?

A: The reaction takes place in the solution prepared by mixing HNO3 and NH3 solutions is written…

Q: Calculate the pH of the resulting solution when 30.0 mL of 0.500M HBr is added to 25.00 mL of 1.00 M…

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Q: С. What is the pH if 25.0 mL of a 0.10 M NaOH solution is added instead of the HCI(aq)?

A:

Q: A solution is made by dissolving 0.06100 moles of Ba(OH)2 in enough water to make 250.0 mL of…

A: Given, moles of Ba(OH)2 = 0.06100 moles Volume of the solution = 250.0 mL = 0.250 L pH of the…

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: Calculate the pH of the acid solution after the chemist has added 51.3 mL of the KOH solution to it.

A:

Q: if 65ml of 0.25M naoh are combined with 76ml of 0.3M h2so4 .What is the pH if the solution is…

A: Given  Millimoles of H2SO4 = M x V = 0.3 x 76  = 22.8 mmol Millimoles of H+ ion = 2 x millimoles of…

Q: What is the pH of solution prepared by mixing 30.0 mL of a 0.40 M HCl(aq) with  20.0 mL of a 0.60 M…

A:

Q: Calculate the pH of (a) 0.050 M HCI(aq) and (b) 0.100 M KOH(ad).

A: negative logarithem of H+ ion concentration is called pH pH = - log[H+]  Similarly  pOH = - log[OH-]…

Q: Calculate the pH when (a) 24.9 mL and (b) 25.1 mL of 0.100 M HNO3 have been added to 25.0 mL of…

A: Part a: Number of moles of nitric acid = 0.0249 L × 0.1 M = 0.00249 mol Number of moles of KOH =…

Q: 30 ml of a 0.4375 M HCl solution are added to 35 ml of 0.250 NaOH solution. What is the final pH ?

A: given :-  molarity of HCl solution = 0.4375 M  volume of HCl solution = 30 mL  molarity of NaOH…

Q: Determine the pH of a solution that results when 15.0 mL of 2.00 mol/L NaOH is added to 25.0 mL…

A: This question belong to ionic equilibrium. pH calculation of mixture of strong acid and strong base.…

Q: Calculate the pH of the resulting solution if 31.0 mL of 0.310 M HCl(aq) is added to 21.0 mL of…

A: pH is a measure of hydrogen ion concentration. The mathematical equation to calculate pH is given…

Q: Calculate the pH of the resulting solution if 25.0 mL of 0.250 M HCI(aq) is added to 30.0 mL of…

A:

Q: If 5.00 mL of 6.00M HCl is added to 95.00 mL of purewater, the final volume of the solution is…

A: If 5.00 mL of 6.00M HCl is added to 95.00 mL of pure water, the final volume of the solution is…

Q: Calculate the pH of a solution prepared from 0.200 mol of NH4CN and enough water to make 1.00 L of…

A: NH4CN is a salt of weak acid HCN and weak base NH4OH. pH of a salt of weak acid (WA)and weak base…

Q: Calculate the pH of the resulting solution if 27.0 mL of 0.270 M HCl(aq) is added to 17.0 mL of…

A: Some of the HCl is neutralized by NaOH. And the remaining HCl will contribute to pH.

Q: Suppose a 0.10OM solution of each of the following substances is prepared. Rank the pH of the…

A: There are some substance :-  KF, NH4I ,HBr, NaCl, LiOH . We have to calculate the PH of the  0.100M…

Q: Calculate the pOH adn the pH of a solution in which 100.0 mL of 0.1500 M HCI is added to 250.0 mL of…

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Q: Calculate the pH of a solution when 20 mL of a 0.125 M HCl are mixed with 20 mL of a 0.050 M…

A: The balanced reaction is: 2HCl + Ba(OH)2  → BaCl2 + H2O To neutralize 1 mol of Ba(OH)2, we need 2…

Q: Calculate the pH of the following solution at 25 °C for which the substance ionizes completely:…

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Q: Do a 1.0 M CH,COOH solution and a 1.0 M HCI solution have the same pH? Explain.

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 of a solution prepared by adding 250 mL of 0.0125 M HNO3 to 500.0 mL of 0.0200 M…

A: Acid is defined as a substance that releases hydronium ion when dissolved in water. Acid is…

Q: If 215 ml of a .01M HBr is reacted with 250 ml of a .007M solution of KOH, what is the resulting pH?

A: HBr    +      KOH            →           KBr  +  H2OINITAL         215×.01…

Q: Lalculate the pH of the resulting solution if 29.0 mL of 0.290 M HCI(aq) is added to 39.0 mL of…

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Q: the pH when15 mL of 0.25 M HClO4 are added to 25 mL of 0.20 M NaOH.

A:

Q: a) How many milliliters of 0.150 M NaOH solution are required to titrate 40.0 mL of a 0.100 M HNO2…

A: a) At the equivalence point, the moles of the solution are equal that is- M1V1=M2V2 where M1:…

Q: Calculate the pH when 35.0 mL of 0.150 M HNO3 is mixed with 40.C mL of 0.250 M LIOH.

A:

Q: Calculate the pH of a solution prepared by mixing 100 ml of 0.1 M HNO3(aq) with 30 ml. of 0.2 M…

A: The reaction taking place between strong acid, HNO3 and strong base LiOH is- Thus, 1 mole of HNO3…

Q: Calculate the pH of a solution made by diluting 11 mL of a 3 M solution of HCI to a final volume of…

A: Initial Molarity of HCl solution = M1 = 3 MInitial Volume of HCl solution = V1 = 11 mL= 0.011 LFinal…

Q: Calculate the pH of each of the following solutions. a. 0.12 MKNO2 b.0.45 MNaOCl c. 0.40 MNH4ClO4

A: The question is based on the concept of salt hydrolysis. we have to calculate pH of the solution.…

Q: Calculate the pH of the resulting solution when 70.00 mL of 1.000 M HCI is mixed with 65.00 mL of…

A: We have to calculate the pH of resulting solution.

Q: Calculate the pH of a solution which results from the mixing of 50 ml of 0.3 M HCI with 50 ml of 0.4…

A: Given volume of HCl = 50 mL = 0.050 L  As, 1000 mL = 1.0 L  Molarity of HCl = 0.3 M = 0.3 mol/L…

Q: A 1.57 M solution of a weak acid HA is found to have a pH of 2.05.     Determine the pH of a 2.00 M…

A: The concentration of hydrogen ions can be calculated as follows-

Q: A solution is made by dissolving 0.05700 moles of Ba(OH)2 in enough water to make 330.0 mL of…

A:

Q: Calculate the pH when 63.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: The reaction taking place can be written as, => KOH + HBrO ------> KBrO + H2O Given :…

Q: Calculate the pH of the resulting solution

A: Given:-  volume of HCl solution = 32.0 mL  molar concentration of HCl solution = 0.320 M  volume of…

Q: When 15.00 mL of 0.0500 M HBr is added to 7.50 mL of 0.100 M LIOH, what is the pH of the resulting…

A:

Q: What is the pH of a solution made by mixing 1.57E1 mL of 0.100 M NaOH(aq) with 50.0 mL of 0.100 M…

A:

Q: When 10 mL of 0.1 M NaOH is added to 50 mL of 0.05 M HCl solution, which is the final pH of the…

A: A numerical problem based on pH determination, which is to be accomplished.

Q: )What is the pH of a solution composed from 52.0 mL of 0.128 M HCI with 48.0 mL of 0.235 M NaOH?

A:

Q: A sample of 0.0084 mol of HCl is dissolved into a solution with total volume of 1500.0 mL. Calculate…

A: Solution stoichiometry involves the calculation of concentration of solutions in the given…

Q: Calculate the pH of the resulting solution if 31.0 mL of 0.310 M HCl(aq) is added to 41.0 mL of…

A: Given : Concentration of NaOH = 0.310 M Concentration of HCl = 0.310 M Volume of HCl solution = 31.0…

Q: What is the pH of the resulting solution if 25.0 mL of 1.12 M HCl is mixed with 60.0 mL of 0.25 M…

A:

Q: Calculate the pOH and the pH of a 0.400 M Ba(OH), solution.

A: We have to predict the pOH and pH of solution.

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.