You combine 50.0 mL of 0.500 M NaOH with 75.0 mL of H2S04 with a Molarity of 0.19598. What is the resulting pH of the solution?

Q: You have a 1.25 L solution with 2.14 g of NaIO and the pH is 11,32. What is the Kb of NaIO?

A: Solution pH, pKa, pKb, Ka, and K ar employed in chemistry to explain however acidic or basic an…

Q: Enter your answer in the provided box. Determine the pH of a solution that is 0.15 M CH3COOH and…

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Q: In the laboratory, a general chemistry student measured the pH of a 0.453 M aqueous solution of…

A: The dissociation of acetic acid is given as, CH3COOH↔CH3COO- + H+ By definition, the acid…

Q: What is the pH of a 0.0520 M solution of HONH,CI (Kb of HONH, is 1.1 × 10*)? 2

A: Solution :      Weak bases show partial ionization on dissociation in an aqueous solution. Here…

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: an aqueous solution containing 3 grams of CH3COOH in 500 ml of it and having a pH = 3 solution of…

A: Given that,  pH of 500 mL solution containing 3 g CH3COOH = 3 Molarity of CH3COOH solution = (3…

Q: You have a 0.0685 M solution of Ca(OH)2, what is the pH of your solution?

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Q: What is the pH of a solution that is prepared by adding 4.0 mL of 0.50 M NAOH(aq) and 4.0 mL of 0.40…

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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: The pOH of an aqueous solution of 0.428 M acetylsalicylic acid (aspirin), HC9H7O4, is

A: Aspirin is a monoprotic weak acid with formula HC9H7O4. Hence it will dissociate partially as per…

Q: The pH of a 0.550 M of weak base, A-,  is 9.93 at 25. What is the Kb of the base?

A: Since the base given is a weak base. Hence it will undergo partial ionisation as per the below…

Q: 0.60 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 6.0 L of solution. What is…

A: Molecular weight of NaOH= (23+16+1) = 40 gm/mol  Amount of NaOH taken = 0.6 gm  Moles of NaOH =…

Q: The pH of an aqueous solution of 0.522 M benzoic acid, C6H5COOH is

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Q: A student is provided with a 1.0 M stock solution of hydrochloric acid (HCl) and asked to mix 5.00…

A: The dilution solution is prepared by reducing the concentration of solute in stock solution by…

Q: Given a mixture of 100cm3 of 1.01M HCl and 400cm3 of 0.04 NaOH, calculate the pH of the solution.

A: We have given that Volume of HCl = V1 = 100ml Molarity of HCl = M1 = 1.01M Volume of NaOH = V2…

Q: In the laboratory, a general chemistry student measured the pH of a 0.564 M aqueous solution of…

A: Quinoline is a heterocyclic aromatic compound and a colorless liquid with a strong odor. Quinolines…

Q: A student added 1.78g of Ca(OH)2(9) to 0.250 L of 0.200 molL"' HNO3(aq)- The mixture was carefully…

A: We have to calculate the pH of solution.

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: The pH value of the 5L aqueous solution prepared with 6.4 grams of a precious strong acid is 2. So…

A: Given, volume of acid solution = 5L Mass of acid = 6.4 g PH = 2  Molar mass of acid = ?

Q: The ph of 168 mL of a .556 M solution of unknown weak base is 12.96. what is the Kb of this base?

A: Volume of solution =168 mL Concentration of solution=0.556 M pH =12.96 Kb=?

Q: If we combine 40.0 mL of a 0.100 M HNO3 solution with 60.0 mL of a 0.100 M ethylamine solution, what…

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Q: If the molar concentration of OH- is 1.0 x 10-7, the pH is what?

A: Applying formula of pH  POH= -log[OH-]

Q: Assume 125.0 mL of the solution prepared above was put into a beaker and 82 mg of NaOH was added to…

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Q: The concentration of CH3COOH (pKa=4.75) in vinegar is about 1.0 M. With this what do you predict the…

A: pH is the negative logarithm of Hydrogen ion concentration. pH of a solution can be calculated as:…

Q: what ph does a 12,7 M NaOH solute have?

A: NaOH ---> Na+ + OH–  [NaOH] = 12.7 M = [OH–]  So, pOH  = – log [OH–] pOH = – log (12.7) = 1.103…

Q: A solution with a volume of 250.0 mL, contains 1.47 g NH, and 3.95 g NH,NO, . a. What is the pH of…

A: The molarity of NH3 and NH4NO3 is: Molarity of NH3 =1.47 g17.03 g/mol×1000250 mL=0.345 MMolarity of…

Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…

A: The dissociation of formic acid. Given data: Initial concentration of formic acid is 0.558M. pH of…

Q: 5 mg of HNO3, which is a strong acid, is added to 750 ml of water. What is the final pH of the…

A:

Q: when 100 ml of a .01 M Mg(OH)2 solution is mixed with 100 mL of a .01 M HCl solution, what is the pH…

A: Since both acids and base are strong  hence they will react to form water as shown below Mg(OH)2 + 2…

Q: . Calculate the resulting pH when 1.00 L of 1.00 M H,SO4 is added to a tank containing 1.00 × 107 L…

A: The dilution of base solution increases the volume of solution and also alter the molarity of…

Q: Determine the base ionization constant (in x 10^5) of a 0.0925 g sample of week base (molar mass =…

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Q: Consider, barium hydroxide, Ba(OH) 2 , a white powdery substance used in the treatment of wastewater…

A: pH is defined as negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L.…

Q: What is the pH of a solution that is prepared by adding 4.0 mL of 0.50 M NAOH(aq) and 4.0 mL of 0.40…

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Q: How many moles of nitric acid do you have in a 0.650 L solution of 0.035 M nitric acid? What is the…

A: Given Data :  Nitric acid molar conc. = 0.035 M Volume of nitric acid = 0.650 L Mole of nitric acid…

Q: The pOH of an aqueous solution of 0.591 M phenol (a weak acid), C,H5OH, is

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Q: How many moles of NH3  would need to be added to 512.9 mL of a 0.25 M solution of NH4Cl to produce a…

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Q: If 10 mL of 0.1 M hypothetical acid, HA, is added with 10 mL of 0.1 M of the salt of its conjugate…

A: Answer: The mixture of acid HA and its conjugate base XA will be a buffer solution.

Q: .623 g of NaC2H3O2 are placed in a solution of 0.105 M HC2H3O2 to make 1.00 L of solution. What is…

A: pH is negative logarithm of Hydrogen ion concentration

Q: A 0.150 M solution of a weak base has a pH of 9.65. What is the base hydrolysis constant, K, for the…

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Q: A reaction requires the addition of 350.0 mL of a solution with a pH of 3.50. What mass of HNO3 (in…

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration of a solution expressed…

Q: If titrating 25.00 mL of 0.115 M HCl with 0.0955 M NaOH, what is the pH of the solution after 10.48…

A: Given:Volume of HCl = 25.00 mLMolarity of HCl = 0.115 MMolarity of NaOH = 0.0955 MVolume of NaOH…

Q: The pH of a solution of M(OH)2 is 13.08 .  What is the molarity of the M2+ ion?

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Q: The pOH of an aqueous solution of 0.590 M phenol (a weak acid), C6H5OH, is _____

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Q: How many grams of NaHCO3 must be added to 4 g K2CO3 to give a pH of 10.80 in 500 ml total solution?

A: Henderson-Hasselbach equation is given by: pH = pKa + logA-HAwhere [HA] is the concentration of the…

Q: E. Calcuiate the pH of a soltition made up by adding0.100g of NaOH to 250.0 mL of a 0.200 M solution…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: 0.50 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 4.5 L of solution. What is…

A: In order to calculate pH of the given base sodium hydroxide, follow the below mentioned steps: 1)…

Q: A solution is prepared by adding 0.10 mol of sodium fluoride, NaF, to 1.00 L of water. What is the…

A: Answer: pH of the solution is 8.09.

Q: A CHM 122 student combines 42.2 mL of 0.413 MHBR with 32.7 mL of 0.384 M KOH. What is the pH of the…

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Q: How many moles of (CH3)3N  would need to be added to 459.2 mL of a 0.25 M solution of (CH3)3NHCL  to…

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Q: Explain how a set of weak bases, all with approximately the same 0.1 molarity, can have different pH…

A: Answer

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.