A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 360. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 97.4 mL of sodium hydroxide solution. Calculate the molarity student's sodium hydroxide solution. Round your answer to 3 significant digits. of the

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A: We calculate normality of acid and base then use this formula N1V1 = N2V2

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…

A: In the given question we have to calculate the Molarity of NaOH solution,  first of all, we have to…

Q: A 150.0 mL solution of 3.011 M strontium nitrate is mixed with 210.0 mL of a 3.176 M sodium fluoride…

A:

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…

A: The reaction of oxalic acid and NaOH is: H2C2O4 +2NaOH →Na2C2O4 + 2H2O

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A: Since the potassium hydrogen phthalate is a monoprotic acid. hence it will have only 1 mole of…

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Q: It is desired to neutralize a solution X that contains a mixture of potassium chloride and…

A: The solution contains several steps.Explanation:Step 1:Step 2: Step 3: Step 4:

Q: mg of OXallo acid (H,C,04), a diprotic acid that can be purchased inexpensively in high purity, and…

A:

Q: A 50.0 mL sample of potassium hydroxide is transferred to an Erlenmeyer flask and then titrated with…

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Q: A 21.88 mL portion of a 0.379 M solution of hydrochloric acid, a monoprotic acid, is to be titrated…

A: Here we are required to find the volume of KOH required to reach the equivalence point.

Q: A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 99.50 mL of 1.500 M NaCl, and the PbCl₂…

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Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…

A:

Q: You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen…

A: Here we are using KHP (1.55 g) to standardize NaOH solution.  After standardization of NaOH…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…

A: We have to calculate the Molarity of NaOH solution.

Q: n analytical chemist weighs out 0.105 g of an unknown monoprotic acid into a 250 mL volumetric flask…

A: At equivalence point mole of standard solution is equal to the mole of unknown solution.

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A:

Q: concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue…

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Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs…

A: First, we need to calculate the number of moles of oxalic acid (H2C2O4) used. The molar mass of…

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A: As most base solutions are secondary standardized, so we need to standardise base solutions with a…

Q: A student titrates a 15.00 mL sample of unknown sodium hydroxide using a standardized 0.12807 M…

A: Volume of NaOH (V1) = 15.00 mL Concentration of HCl (M2) = 0.12807 M Initial volume of HCl = 1.26 mL…

Q: An unknown amount of acid can often be determined by adding an excess of base and then…

A: The number of protons obtained from the mixture are,

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: To a 25.00 mL volumetric flask, a lab technician adds a 0.200 g sample of a weak monoprotic acid,…

A: The reaction for the process is given below : HA  +  KOH  →  KA  +  H2O Given data : Concentration…

Q: An analytical chemist weighs out 0.123 g of an unknown monoprotic acid into a 250 mL volumetric…

A:

Q: Consider a titration where 0.215 M potassium hydroxide is added from a burette to 10.00 mL of…

A: Given information,

Q: By titration, it is found that 58.5 mL of 0.177 M NaOH(aq) is needed to neutralize 25.0 mL of…

A:

Q: What was the molarity of the KOH solution

A: Molarity = number of moles/volume of solution (in L)   Number of moles = molarity x volume

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…

A:

Q: A 185.0 mL sample of 1.200 M Pb(NO₃)₂ is mixed with 119.50 mL of 1.500 M NaCl, and the PbCl₂…

A: The balanced Chemical Reaction for less Nitrate and sodium chloride is - Pb(NO₃)₂  + 2NaCl ---->…

Q: You have been provided with a 2.13 x 10-2 L  sample of lithium hydroxide (LiOH) of unknown…

A:

Q: An acid-base titration is used to standardize a solution of NaOH. A student adds 25.00 mL of a…

A: KHP + NaOH→NaKP + H2O At equivalence point No. of moles of KHP=No. of moles of NaOH

Q: A chemistry student weighs out 0.166 g of ascorbic acid (H,C,H,O), a diprotic acid, into a 250. mL…

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Q: The concentration of HCl can be determined by titration with a primary standard such as sodium…

A: First calculate the moles of Na2CO3: moles of Na2CO3 = Mass/Molar mass = 0.421g/(106gmol-1) = 3.97 ×…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…

A: First, we need to calculate the number of moles of oxalic acid (H2C2O4) used. The molar mass of…

Q: A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs…

A:

Q: An analytical chemist weighs out 0.127 g of an unknown monoprotic acid into a 250 mL volumetric…

A: Given:-analytical chemist weighs = 0.127 gMolarity = 0.1800MV = 9.3 mLCalculate molar mass of the…

Q: The titration of 25.0 mL of an iron(II) solution required 18.0 mL of a 0.115 M solution of…

A: Net ionic equation for the reaction between iron(II) and dichromate is shown below. Number of moles…

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for