To increase the acidity of soil you can add peat, which contains a complex diprotic acid known as humic acid. The complexity of humic acid makes it difficult to determine how acidic you are making the soil, so you decide to use a titration to get a better measure. You dilute 1.00 mL of your standardized sodium hydroxide in a 100 mL volumetric flask. A 50.0 mL extraction of peat requires 7.51 mL of your dilute sodium hydroxide. What is the concentration (in mM) of humic acid in the peat

Q: If you find that a 69.8 mL sample of vinegar requires 120.31 mL of a 0.504 M solution of NaOH for…

A: To calculate the amount of acetic acid in the vinegar sample, we can use the following balanced…

Q: A chemist weighs out 0.138 grams of an unknown diprotic acid into a 222 volumetric flask and makes a…

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

Q: An analytical chemist weighs out 0.054 g of an unknown monoprotic acid into a 250 mL volumetric…

A:

Q: An analytical chemist weighs out 0.203 g of an unknown diprotic acid into a 250 mL volumetric flask…

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Q: 30 mL of an unknown concentration of phosphoric acid (triprotic) was titrated with 10 mL 0.05 M…

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Q: A student is trying to determine the molar mass of an unknown weak, monoprotic acid. A solution of…

A:

Q: 10.A 0.1268 g sample of a monoprotic weak acid was dissolved in 25 mL of water and titrated with…

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Q: The buret is filled with 0.1475 M NaOH. The beaker has 25.00 mL of 0.1276 M HCl. Predict what…

A: Solution:

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A: Molarity is the number of moles of solute present per litre of solution.

Q: A titration flask contains 0.00405 moles of an acetic acid sample   a. Determine the moles of the…

A: The given number of moles of acetic acid is 0.00405 mol. The molarity of NaOH is 0.200 M. The…

Q: An analytical chemist weighs out 0.165 g of an unknown triprotic acid into a 250 mL volumetric flask…

A: The unknown acid is triprotoic acid, hence the balanced chemical reaction between the acid and NaOH…

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Q: A group of students working in a chemistry lab is planning a procedure to neutralize 25.0mL of 2.0 M…

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Q: A student titrates a weak acid with 0.100 M NaOH, adding 31.65 mL before a dark pink color is seen.…

A: The mole of H+ ion the weak acid is equal to the mole of NaOH used in the titration.  The molarity…

Q: In a titration, suppose 20.00 mL of 0.275 M oxalic acid solution required 21.72 mL of NaOH solution…

A: H2C2O4(aq) + 2NaOH(aq) -------> Na2C2O4(aq) +2H2O(l)

Q: A 0.0892 M solution of sodium hydroxide was used during a titration to determine the concentration…

A: Given, Molarity of NaOH , M1 = 0.0892 M Volume of NaOH , V1  = 22.50 mL  Volume of HNO3 , V2 = 15.00…

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A:

Q: Suppose you are titrating an acid of unknown concentration with a standardized base. At the…

A: Initial volume reading of the burette = 2.31 mL Final volume reading of the burette = 22.53 mL…

Q: An analytical chemist weighs out 0.102 g of an unknown diprotic acid into a 250 mL volumetric flask…

A:

Q: A 35.00 mL volume of formic acid is titrated with 0.1428 M potassium hydroxide (KOH). If 24.39 mL…

A: Given: The concentration of potassium hydroxide (KOH)=0.1428 M The volume of potassium hydroxide…

Q: A solution of oxalic acid is used to titrate 17.11 mL of a 0.5003 molar: sodium hydroxide. If the…

A:

Q: An analytical chemist weighs out 0.461 g of an unknown triprotic acid into a 250 mL volumetric flask…

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Q: The iodine contained in every one mL of the 0.010 M iodine solution in the buret will react with…

A: Given, volume of titrant, iodine solution used = 5.14 mL            mass of vitamin C titrated by 1…

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Q: 2. In an acid base titration 37.45 mL of barium hydroxide were neutralized by 45.65 mL of 0.250 M…

A:

Q: A student titrates a weak acid with 0.100 M NaOH, adding 34.84 mL before a dark pink color is seen.…

A: Calculation of no. of mol of NaOH: No. of mol=Molarity×Volume=0.100 mol/L×34.84×10-3 L=3.484 ×10-3…

Q: unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which…

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Q: A 13.8 mL solution of 0.176 M phosphoric acid (aq) is to be titrated with 0.384 M sodium hydroxide…

A: The mathematical calculation can be explained using acidimetry and alkalimetry . From this principle…

Q: An analytical chemist weighs out 0.278 g of an unknown diprotic acid into a 250 mL volumetric flask…

A: Given-> Weight of diprotic acid = 0.278 gm Volume of flask= 250 ml = 0.250 L (1 L = 1000 ml)…

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A: Given: In a titration to determine the concentration of hydronium ions in a test solution: The test…

Q: An analytical chemist weighs out 0.066 g of an unknown monoprotic acid into a 250 mL volumetric…

A: Given:-analytical chemist weighs = 0.066 gMolarity = 0.1700MV = 8.4 mLCalculate molar mass of the…

Q: A 30.00 ml sample of phosphoric acid is titrated with a 0.050 M magneisim hydroxide solution.  The…

A: Given: Volume of sample = 30.00 mLInitial buret reading = 4.71 mLFinal buret reading = 31.09…

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Q: When a 17.2 mL sample of a 0.311 M aqueous acetic acid solution is titrated with a 0.327 M aqueous…

A: Here CH3COOH reacts with Ba(OH)2. Reaction is - 2 CH3COOH + Ba(OH)2 = (CH3COO)2Ba + 2 H2O Using…

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Q: If the concentration of the NaOH that was added was 1.0 M and the volume of oxalic acid being…

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Q: A 24.5 mL sample of vinegar is titrated with 0.451 M NaOH(aq). If the titration requires 33.0 mL of…

A:

Q: An analytical chemist weighs out 0.203 g of an unknown diprotic acid into a 250 mL volumetric flask…

A: l

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A: This problem can be solved by using molarity equation which may be expressed as ; M1V1=M2V2

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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.