A compound has a place of 7.4. To 100mL of 1.0 solution of this compound at 8.0 is added 30mL of 1.0 M hydrochloric acid. What is the pH of the resulting solution?

Q: 50 mL of 0.02 M NaOH is added to 25 mL of 0.04 M HCl solution. The pH of the resulting solution will…

A: Balanced chemical equation: NaOH (aq)  +   HCl (aq)   ------->  NaCl (aq)  +  H2O (l) Number of…

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: A solution is prepared that is initially 0.092 M in methylamine (CH,NH,), a weak base, and 0.10 M in…

A: Given data: A solution is prepared that  initially contain 0.092 M in methylamine (CH3NH2 ),a weak…

Q: Determine the pHof a solution prepared by dissolving 35.0g of solid (CH3)NH2CL in 1.00L of 1.10M…

A: At equilibrium (CH3)2NH hydrolyzes as,                                            (CH3)2NH + H2O ⇌…

Q: A solution is prepared that is initially 0.17 M in trimethylamine ((CH,) N), a weak base, and 0.20 M…

A: In this question, we have to find out the correct answer of given problem by the help of the…

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: b) To 1 L of the solution in part (a) are added 0.010 moles of solid Sodium Hydroxide (which…

A: This can be solved by finding the concentration of that base and acid. That can be solved by…

Q: 50.00 mL of 0.200 M sodium dihydrogen pyrophosphate (N22H2P207) solution is combined with 25.00 mL…

A: Buffer solution is prepared, when an strong base is added into weak acid solution then resulting…

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: An aqueous solution contains 0.461 M ammonla. Calculate the pH of the solution after the addition of…

A: The concentration of ammonia = 0.461 M = 0.461 mol/L (M = mol/L) The number of moles of hydrobromic…

Q: Acid dissociation constants for sulfurous acid are given below. Solution A and Solution B are mixed.…

A: Given data,Molarity of KHSO3=1.00MVolume of KHSO3=200mLMolarity of KOH=1.00MVolume of KOH=40mL

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: 210 ml of 0.10 M hydroiodic acid, HI, is mixed with 100.0 ml of 0.10 NaOH. Determine the pH of the…

A: Hl is a strong acid and NaOH is a strong base. They react in 1:1 molar ratio as below : HI + NaOH…

Q: A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

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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: An aqueous solution of 0.1 M hydrochloric acid with a volume of 200 milliliters is mixed with 100 mL…

A: Moles of HCl taken = molarity of HCl X volume of HCl solution taken in L Since molarity of HCl = 0.1…

Q: Calculate the pH of the solution that results when 32.0 mL of 0.1980 M NH3 is (This problem requires…

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Q: 8) Given a buffer solution that is 0.250 M in formic acid (HCOOH) and 0.150 M sodium formate…

A: From given data  Formic acid concentration [Acid]= 0.250 M Sodium formate concentration [Salt]=…

Q: A solution is prepared that is initially 0.36M in trimethylamine ((CH3),N), a weak base, and 0.19M…

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Q: 25.00ml of 0.5M hydrobromic acid solution is titrated with 0.455M potassium hydroxide solution. what…

A: A neutralization reaction can be described as a chemical reaction in which acid and base reacts…

Q: 1. 25.00 mL of 0.2M acetic acid and 3.81 mL of 0.20 M NaOH were mixed together. The resulting…

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Q: A solution is made by combining 25.00 mL of 0.15 M sodium hydrogen phosphate and 15.00 mL of 0.15 M…

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Q: Calculate the pH of a 0.50 M HCOOH/ 0.60 M HCOOK buffer solution, and calculate the pH when 5.00 mL…

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Q: The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with…

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Q: A 100.0 mL of 0.1 M HCI solution is mixed with a 50.0 mL of 0.1 M of KOH solution. The resultant…

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Q: Calculate the pH of solution prepared by dissolving 0.10 mol of NH.Cl and 0.40 mol of NH; in…

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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: I prepare a buffer solution by mixing 30.0mL of 0.10M HOAc and 40.0mL of 0.10m NaOAc. I divide this…

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Q: 50.0 mL of 0.100 M HBr(aq) is mixed with 50.0 mL of 0.0800 M KOH(aq). What is the pH of the final…

A: No. of mmol of HBr = 50 mL× 0.1M= 5mmol No. of mmol of KOH = 50 mL ×0.08M = 4 mmol

Q: A solution containing 15.0mL of 4.00MHNO3 is diluted to a volume of 1.00L. What is the pH of the…

A: The given volume and molarity of HNO3 are 15.00 mL and 4.00 M. The given volume of diluted solution…

Q: Solution Measured pH Theoretical [H30*| |Calculated pH Distilled water 7.10 Original buffer solution…

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Q: Calculate the pH when 29.91 mL of 0.2628 M carbonic acid is mixed with 10.1 mL of 0.1448 M NaOH.

A: For carbonic acid, 29.91 mL of 0.2628 M carbonic acid Ncarbonic acid  = n- factor × M…

Q: Calculate the expected pH based on how the solution was prepared, again allowing for any dilution…

A: pH of a buffer solution can be calculated by using Henderson Hasselbalch equation, according to…

Q: An aqueous solution contains 0.443 M ammonia. Calculate the pH of the solution after the addition of…

A: The reaction takes place as follows: NH3 + HI ⇌ NH4+ + I- Volume of ammonia=155 mL=0.155 L Moles of…

Q: Explain how the pH of a mixture of aqueous ammonium chloride and aqueous ammonium remains constant…

A: The solution that can resist the addition of the strong acid or strong base is termed as the buffer…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.11 M solution. The pH of the…

A: The concentration H3O+ of weak acid [H3O+] = Ka*C  where Ka is the dissociation constant, C is the…

Q: 10010 ml, 0.1M HcL is udded to 100 ml of asalFion Which IS 0.1 M both in HOAC and NAOAC. By how many…

A: The questions are based on the concept of PH calculations. we have to determine how much by pH…

Q: 100ml of solution contains 0.4 gm caustic soda. in dissolved state. If 50ml of this solution is…

A: Caustic soda is NaOH with molar mass = 40 g/mol Hence moles of NaOH taken X molar mass of NaOH =…

Q: A compound has a pKa of 7.4. To 100 mL of a 1.0 M solution of this compound at pH 8.0 is added 30 mL…

A: The pH is the measure of the acidity of the solution. The Henderson-Hasselbalch equation calculates…

Q: Calculate the pH of a 0.5 Litre solution wich prepared by adding (50ml NH3) to a sufficient amount…

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Q: 200 mL of 0.1 M HCl is added to 400 mL of 0.1 M sodium acetate and water is added to give a final…

A: A buffer solution is the one which is made by adding a weak acid with its conjugate base. Any slight…

Q: A solution was prepared by mixing 50.0 mL of 0.10 M HCl and 25.0 mL of 0.25 M NaOH. What is the pH…

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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…

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Q: A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

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Q: An alkaline solution was prepared with LiOH in such a way that 0.65 g dry LiOH was directly mixed…

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Q: Enough of a monoprotic acid is dissolved in water to produce a 1.21 M solution. The pH of the…

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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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Q: An aqueous solution contains 0.301 M hydrocyanic acid. Calculate the pH of the solution after the…

A: Given-> Molarity of HCN = 0.301 M Volume of HCN = 125 ml = 0.125 L (1L = 1000ml) Moles of KOH =…

Q: Determine the pH of the resulting solution when the following two solutions are mixed: 30.0 mL of…

A: Step - 1CH3NH2 + HClO3 → CH3 NH3⊕ Salt∵ C = nvWhere,c = concentrationn = no.of molesv = volume∴ n =…

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.