3. Following a standardization reaction, the concentration of an aqueous solution of NaOH is determined to be 0.510 M. a. What is the mass of NaOH in 50.0 mL of this solution? Show your work. b. What mass of KHP would be needed to completely react with 50.0 mL of this NaOH solution? Show your work.

3. Following a standardization reaction, the concentration of an aqueous solution of NaOH is determined to be 0.510 M. a. What is the mass of NaOH in 50.0 mL of this solution? Show your work. b. What mass of KHP would be needed to completely react with 50.0 mL of this NaOH solution? Show your work.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter35: Spot Tests For Some Common Anions

Section: Chapter Questions

Problem 3ASA

See similar textbooks

Related questions

Q: For this exercise, let's say that you begin with an aqueous mixture containing the following…

Q: A sample of hydrated nickel(II) chloride was heated to remove the waters of crystallization. The…

Q: Following a standardization reaction, the concentration of an aqueous solution of NaOH is determined…

A: Given, molarity of NaOH = 0.15 M Volume of NaOH = 50 mL= 0.05 L Molarity = mole/molar mass

Q: Standardization of a sodium hydroxide solution against potassium hydrogen phthalate (204.2 g/mol)…

A: First, calculate the moles of KHP: Moles of KHP = mass/molar mass = 0.8365g/(204.2gmol-1) = 0.004096…

Q: In preparation of cola, 2.50 mL of the original sample was taken and diluted to 100 mL resulting to…

Q: Calculation:Calculate the final concentration of a solution prepared by diluting 1.50 mL of a 20.00…

A: The final concentration of a solution is to be calculated which is prepared by diluting 1.50 mL of…

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

Q: Following a standardization reaction, the concentration of an aqueous solution of NaOH is determined…

A: a.) Given Molarity and volume of NaOH solution , from this we can calculate moles of NaOH. From…

Q: 30.0 cm3 of aqueous sodium hydroxide containing 8.0 g per litre of sodium hydroxide were completely…

A: The reaction of sodium hydroxide with dibasic acid is shown below:

Q: sodium thiosulfate, Na2S2O3,Na2S2O3, solution for a titration experiment. To do so, he or she will…

Q: "Find the molarity of the Na+ ions when 78.0 g Na2S is dissolved in water for a final volume of 1.0…

A: Volume of solution =1.0 L

Q: For the analysis of unknown soda and vinegar samples, 25.0 mL soda and 1.0 mL vinegar samples were…

Q: f 20. g of AgNO3 is available, what volume of 0.40 M AgNO3 solution can be prepared? Volume =…

A: Molarity is the moles of solute per liter volume of solution. It is represented as M.

Q: To make 1.00 L of 1.00 M NaOH solution, what mass of NaOH needs to be weighed out?

A: 1 M NaOH solution means 1 mole NaOH is present in 1000 mL means 1 L solution.

Q: 5 A,B,C,D

Q: Standardization of a sodium hydroxide solution against potassium hydrogen phthalate (KHP) yielded…

A: The chemical reaction between KHP and NaOH is given by - KHP…

Q: PROBLEM STATEMENT: 50 mL of 3.5 m potassium nitrate is added to 50 mL of 3.5 M Aluminum Chloride.…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: What volume (in ml) of concentrated HCl (with a concentration of 10 M) do you need to prepare 10 ml…

Q: Mass of the reaction solution, msoln (g) Add together the masses of the NaOH (100mL) (aq) and HCl…

A: Given, Volume of NaOH = 100 mL Volume of HCl = 100 mL Density of the solution = 1.00 g/mL Mass…

Q: An unknown amount of barium nitrate is dissolved in 120.0 g of water and 8.15 g of copper (II)…

Q: A student, performing the same experiment as you, recorded the following information. The original…

A: The balanced reaction of acetic acid v/s NaOH is as follows: CH3COOH+NaOH→CH3COONa+H2O Determination…

Q: For the analysis of unknown soda and vinegar samples, 25.0 mL soda and 1.0 mL vinegar samples were…

A: During the process of titration, titrant is added to the solution of analyte until the number of…

Q: hydrochloric

A: According to the question, hydrochloric acid solution is standardized with contaminated sodium…

Q: 5. A 0.331 g sample of aspirin prepared in the laboratory was dissolved in 95% ethanol and titrated…

A: a) The number of moles is calculated as, 0.107 M NaOH = mol/ 0.0167 Lmol= 0.107 mol/L x 0.0167 L =…

Q: Standardization of a sodium hydroxide solution against potassium hydrogen phthalate (KHP) yielded…

A: The detailed solution is solved on the white sheets of paper attached below. Here it is important…

Q: An unknown mass of Na;PO4(s) is dissolved in water to form 50.00 mL of solution. This is Solution A.…

A: SOLUTION: Step 1: 1 mole of Na3PO4 contains 3 moles of Na+ ions. 20 mL of solution B contains 4.408×…

Q: When using volumetric flask, why do we have fill it exactly on the given mark? What would be the…

A: The question is based on the concept of solutions. solution preparation is a very important task and…

Q: 43. A 10.00 mL sample of 2.05 M KNO3 is diluted to a vol- ume of 250.0 mL. What is the concentration…

A: As per our honor code we are authorized to solve only one question in one request. We’ll answer the…

Q: Consider a rxn in which Mg metal reacts with Hcl to form aqueous magnesium chloride and hydrogen…

A: We have to calculate the mass of hydrogen gas produced .

Q: To what final volume (L) would you dilute 25.00 mL of 0.250 M NaCl to make a 1.00 × 10-4 M solution?

Q: A sample is reported to contain 44.0% by weight KHP. If you weigh 1.272 g of sample and dilute to…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: This is my second time submitting this question, please help write out equations even if it is just…

A: According to law of equivalence, an acid exactly neutralizes the same number of equivalents of base…

Q: A solution of HNO3 is standardized by reaction with pure sodium carbonate: 2H+ + Na2CO3 → 2Na+ + H2O…

Q: 4. From the information below, determine the mass of NH3 in 500. grams of concentrated ammonia? DATA…

A: Given: Mass of concentrated ammonia= 500 g ℅ mass of solute = 28 ℅ Density of ammonia = 0.90 g/mL

Q: Part A A sample of 7.92 g of Mg(OH)2 is added to 24.2 mL of 0.225 MΗΝΟ, Part B Part C • Part D •…

Q: Q. A 12.5% (w/w) NICI2 (129.6l g/mol) solution has a density of 1.149 g/mL. Calgulate(a) the molar…

Q: Use the following data table and steps a-d below to calculate the concentration of the zinc…

A: Reaction: a) Zn(NO3)2 + Na2CO3 ----> ZnCO3 + 2 NaNO3 mass of filter paper = 1.3457 g mass of…

Q: You dilute the river water 10 times for the analysis of SDS concentration. The instrument measures…

Q: What volume, in mL, of 0.264 M HCl is needed to neutralize 15.0 mL of 0.404 M Sr(OH)2? Express your…

A: Neutralization reaction: The hydrogen ion of an acid reacts with the hydroxide ion of a base to form…

Q: A student adds 10.2 mL of 7.06 M of nitric acid to 0.5502 g copper turnings. What volume of 3.44 M…

Q: (b) An unknown mass of Na3PO4(s) is dissolved in water to form 50.00 mL of solution. This is…

A: The number of moles of Na3PO4 in the 20.00 mL of the solution B is calculated as shown below.

Q: 3. Folldwing a standardization reaction, the concentration of an aqueous solution of NaOH is…

A: We know , Molarity = moles / volume of solution in L By using this realtion we can calculate the…

Q: percent calcium chloride by mass in the original mixture.

A: Given, Mass of a mixture of calcium nitrate and calcium chloride = 1.25 g Volume = 200 mL = 0.200 L…

Q: Normally, the amount of silver nitrate required to precipitate all of the chloride in the sample is…

A: According to the law of chemical equivalence, in a chemical reaction, the number of equivalents that…

Q: A student used a standard silver nitrate solution (0.1050 M) and standard potassium thiocyanate…

A: Calculate the total number of moles of silver nitrate present in the solution.

Q: Case Study - Bottling a Carbonated Drink The process of dissolving carbon dioxide (CO.) in water in…

A: Properties of different substances.

Q: The reaction of NaOH and HCl produces aqueous NaCl as a product. You are assuming that the small…

A: Sodium hydroxide and hydrochloric acid are reacted to give sodium chloride which is salt and water.…

Q: DATA: M standardized NaOH 0.1103 Trial I Trial Trial III 28.52 28.75 28.93 Volume of NaOH added to…

Q: For the analysis of unknown soda and vinegar samples, 25.0 mL soda and 1.0 mL vinegar samples were…

A: Given data,Mass of KHP=0.85gMolar mass of KHP=204.22g/molVolume of NaOH for…

Q: How much water (in mL) should you add to 50.0 mL of 0.300 M H2SO4 (aq) to get a solution of 0.130 M…

A: Given: The initial volume, (Va)=50 mL The initial concentration, (Ma)=0.3 M The final volume,…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

3. Following a standardization reaction, the concentration of an aqueous solution of NaOH is
determined to be 0.510 M.
a. What is the mass of NaOH in 50.0 mL of this solution? Show your work.
b. What mass of KHP would be needed to completely react with 50.0 mL of this NaOH
solution? Show your work.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A student, performing the same experiment as you, recorded the following information. The original solution was diluted by a factor of 5. Calculate the moles of acetic acid in the diluted sample. Volume of diluted vinegar sample (mL) 25.00 Molarity of NaOH 0.0900 Initial buret reading (mL) 16.50 Final buret reading (mL) 38.00 Moles of acetic acid (diluted)
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
This is my second time submitting this question, please help write out equations even if it is just for the 1st sample so I can apply the values for 2 and 3. Please help me understand the equations for this table. How do I calculate the moles of NaOH and acetic acid? How do I calculate the mass of acetic acid? How do I calculate the molarity and % mass of acetic acid. Thanks! moles of NaOH = 1.0 M x 6.2 mL x 1 L/1,000mL = 0.0062 moles NaOH - from lab manual the experimental data is in the picture with blue answers, the second part of the table I need help with.
To dilute 250.0 mL of 1.00 M HCl to a concentration of 0.200 M, what must the final volume of the solution be? To how much additional solvent must the original 250.0 mL of solution be added?
"To what volume should you dilute 0.200 L of 15.0 M NaOH to make 3.00 M NaOH? Make sure to show your work clearly and to the correct number of significant figures". *Please show soltion one step at a time, thank you in advance!
In the first part of this experiment, sodium percarbonate will be dissolved in water: Na2CO3·n H2O2(s) → 2 Na+(aq) + CO32–(aq) + n H2O2(aq) The hydrogen peroxide thus generated will be consumed by iodide and sulfuric acid: H2O2(aq) + 2 H+(aq) + 3 I– → 2 H2O(l) + I3–(aq) Finally, the triiodide anion will be consumed by added thiosulfate: 2 S2O32–(aq) + I3–(aq) → S4O62–(aq) + 3 I–(aq) Considering these chemical equations, if 0.437 millimoles of thiosulfate were needed to completely consume all of the triiodide generated in reaction 2, how many millimoles of hydrogen peroxide were present in the original sodium percarbonate sample?
In the first part of this experiment, sodium percarbonate will be dissolved in water: Na2CO3·n H2O2(s) → 2 Na+(aq) + CO32–(aq) + n H2O2(aq) The hydrogen peroxide thus generated will be consumed by iodide and sulfuric acid: H2O2(aq) + 2 H+(aq) + 3 I– → 2 H2O(l) + I3–(aq) Finally, the triiodide anion will be consumed by added thiosulfate: 2 S2O32–(aq) + I3–(aq) → S4O62–(aq) + 3 I–(aq) Considering these chemical equations, if 0.416 millimoles (mmol) of thiosulfate were needed to completely consume all of the triiodide generated in reaction 2, how many millimoles of hydrogen peroxide were present in the original sodium percarbonate sample? Enter your response to the nearest 0.001 mmol.
1. Use the following data table and steps a-d below to calculate the concentration of the zinc carbonate. The mass of the filter paper alone (no ZnCO3) was 1.3457 g. The Zn(NO3)2 solution (10.00 mL) was mixed with 15.00 mL of the 1.00 M Na2CO3. a. Calculate the mass of zinc carbonate formed. b. How many moles of zinc carbonate formed? c. Calculate the moles of zinc in the zinc nitrate solution used. d. Calculate the concentration of the zinc in the zinc nitrate solution.
VOLUMENTRIC ANALYSIS Instructions: Answer each of the problems below by showing your solutions neatly and logically. Copy and answer each problem and please box your final answers. 4. If a 1.2500 g sample of zinc oxide, 95.0% ZnO were treated with 50.00 mL of 1.1230 N sulfuric acid in the usual way, what volume of 0.9765N sodium hydroxide would be required in the back titration. NOTE: KINDLY WRITE THE SOLUTIONS ON A SEPARATE SHEET OF PAPER
In an impure sample of table salt that weighed 0.8421 g when dissolved in water and treated with excess AgN03 formed 2.044 g of AgCl. Listing the percentage of NaCl is in the impure sample. What is the list of three sources of error in this experiment?
To prepare 50 mL solutions of 0.01 M KMnO4 in water (calculation to prepare chemicals in spectrophotometer)
A student carried out an experiment trying to prepare tetra-methyl-ammonium tri-iodide.The student weighed 1.13 g tetra-methyl-ammonium iodide into a beaker containing 25 mL ethanol, and then added 1.57 g of iodine. The mixture was heated gently, whilst stirring, on a hotplate until tetra-methyl-ammonium iodide, a white powder, was completely dissolved. After the mixture was allowed to cool down to room temperature, the mixture was further cooled on ice. After filtration on a Buechner funnel, washing with diethyl ether and leaving it under vacuum suction for a couple of minutes, the student recovered the product and weighed it. The mass of the obtained tetra-methyl-ammonium triiodide was 1.62 g.What is the yield of the reaction in percent [%]? For the calculation, assume that the product is completely dry and pure, so there are no impurities like side-products, unreacted educts, or solvent residues.