Answered: In the laboratory a student combines…

In the laboratory a student combines 20.5 mL of a 0.177 M sodium phosphate solution with 12.7 mL of a 0.571 M sodium bromide solution. What is the final concentration of sodium cation ? M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A student combined 45.3 mL of a 0.549 M calcium nitrate Ca(NO3)2 solution with 88.20 mL of a 1.321 M…

Q: A student pipet 10.0 mL of an acid solution. They titrated it with 14.82 mL of 1.228M NaOH solution.…

A: Given: Concentration of NaOH solution = 1.228 M Volume of NaOH solution used = 14.82 mL. And volume…

Q: 400.0 mL of a 0.455 M solution of NaCl is diluted to 900.0 mL. What is the new concentration of the…

A: Given, 400.0 mL of a 0.455 M solution of NaCl is diluted to 900.0 mLwe are asked to calculate the…

Q: You wish to make a 0.276 M hydrobromic acid solution from a stoc solution of 3.00 M hydrobromic…

Q: A student titrates an unknown amount of potassium hydrogen phthalate with 26.86 mL of 0.1000 M NaOH.…

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

Q: To make 1.50 L of 0.100 M NaCl from a 2.96 M stock solution, you would need to take mL of the stock…

A: Concentration of stock NaCl solution, M1 is 2.96 M. Volume of stock NaCl solution is V1. Volume of…

Q: What volume of a 0.156 M barium hydroxide solution is required to neutralize 25.6 mL of a 0.126 M…

A: Given Concentration of ba(oh) 2 = 0.156 M Concentration of oh- (M1) =0.156*2 = 0.312 M Concentration…

Q: In the laboratory a student combines 31.8 mL of a 0.232 M sodium sulfate solution with 24.7 mL of a…

A: Number of moles of solute devided by volume of solution in liter is known as molarity.

Q: You wish to make a 0.374 M perchloric acid solution from a stock solution of 12.0 M perchloric acid.…

A: Given a stock solution of 12.0 M perchloric acid. We wish to prepare 50 mL of 0.374 M diluted…

Q: If 400 mL of water is added to 250 mL of a 2.4 M MgCl2 solution, what is the final concentration of…

A: Introduction: Molarity: Molarity is often used to express the concentration of the solution. It is…

Q: A student pours 350 mL of a 6.0 molar solution of sodium hydroxide into a 750 mL volumetric flask…

A: Given data : Initial volume of the solution = 350 mL = 0.35 L Molarity = 6 M So, Number of…

Q: What volume (in ml) of a 12.00M stock solution of HCl is required to prepare 500.00ml of a 3.65…

A: The mass of HCl standard = Density × Volume The mass of HCl standard = 3.65 × 10-3 g/mL × 500 mL =…

Q: 4. What volume of 12.0M HCl stock solution is required to produce 200mL of a 2.50M diluted solution…

A: We have to find, how much volume of stock solution of 12.0 M HCl solution is required to produce 200…

Q: You then titrated a 25.00 mL sample of an unknown HCl solution and it took 33.55 mL of your 0.997 M…

A: HCl is a monoprotic strong acid. NaOH is a monoacidic strong base. Hence 1 mol of each undergo…

Q: 6.0 M HCl solution must be diluted to 0.50 M. If the diluted solution has a total volume of 300.0…

A: Assuming V mL of the concentrated HCl is needed Since the process is dilution hence the moles of…

Q: 300.0 mL of a 0.360 M solution of Nal is diluted to 700.0 mL. What is the new concentration of the…

Q: Imagine you transferred 5.00 mL of 1.75 M HCl solution into an empty 200.00 mL volumetric flask then…

A: Given is Initial Volume of HCl solution = V1 = 5 mL Molarity of HCl solution = M1 = 1.75 M Final…

Q: An aqueous solution of barium hydroxide is standardized by titration with a 0.121 M solution of…

Q: What volume (in mL) of 5.65 M HCl can be made by mixing 6.55 M HCl with 424 mL of 4.45 M HCl?

A: The 5.65 M HCL solution is made by mixing 6.55 M HCl with 424 mL of 4.45 M HCl. The volume of 5.65…

Q: You wish to make a 0.115 M perchloric acid solution from a stock solution of 3.00 M perchloric acid.…

A: The given problem can be solved by using the formula given below as; M1 V1 = M2 V2…

Q: 37.50 mL of a diprotic acid solution, whose concentration is unknown, is titrated with 12.54 mL of…

A: Given that, Volume of diprotic acid V1 = 37.50 mL Concentration of diprotic acid M1 = ? Volume of…

Q: In the laboratory you dilute 4.26 mL of a concentrated 3.00 M hydrobromic acid solution to a total…

Q: A 25 ml aliquot of a 2.00 M stock solution is placed in a 300. mL volumetric flask. When it is…

A: Given that, M1=2.00M , V1=25 mL M2=? , V2=300mL

Q: What volume of a 0.243 M hydrochloric acid solution is required to neutralize 20.7 mL of a 0.175 M…

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

Q: You wish to make a 0.149 M hydrochloric acid solution from a stock solution of 6.00 M hydrochloric…

A: Calculate the number of moles of HCl in the final dilute solution of 0.149 M and 50.0 milliliters.

Q: In the laboratory a student combines 22.2 mL of a 0.138 M sodium carbonate solution with 28.8 mL of…

A: Hello. Since your question has multiple parts, we will solve the first question for you. If you want…

Q: In the laboratory a student combines 29.1 mL of a 0.171 M silver acetate solution with 21.7 mL of a…

A: Given: Concentration of silver acetate i.e. CH3COOAg = 0.171 M Volume of CH3COOAg solution = 29.1 mL…

Q: What mass of sodium chloride will you need to weigh out

A: Molarity = number of moles of solute/volume of solution (in L)/ so, number of moles = molarity ×…

Q: A 10.0 mL sample of an HCl solution is titrated with a 1.00 M NaOH solution. The neutralization…

A: For NaOH solution, Concentration of NaOH solution = 1.00 M = 1.00 mol/L Volume of NaOH solution =…

Q: In the laboratory a student combines 43.2 mL of a 0.275 M lead nitrate solution with 14.9 mL of a…

A: Information about the question

Q: An aqueous solution of barium hydroxide is standardized by titration with a 0.174 M solution of…

Q: In the laboratory a student combines 46.1 mL of a 0.375 M silver acetate solution with 16.1 mL of a…

A: The objective of the question is to find the final concentration of acetate anion when a silver…

Q: Chemistry labs often purchase concentrated HCl (12.0 M) and dilute the solution for laboratory use.…

A: Molarity of initial solution = 12.0 M Molarity of new solution = 0.250 M Volume of new solution =…

Q: An aqueous solution of barium hydroxide is standardized by titration with a 0.109 M solution of…

Q: In the laboratory a student combines 46.6 mL of a 0.307 M iron(III) fluoride solution with 22.4 mL…

A: GIVEN: The Volume of Iron(III) Fluoride = 46.6 mL The concentration of Iron(III) Fluoride =0.307 M…

Q: What volume of a 0.135 M calcium hydroxide solution is required to neutralize 19.1 mL of a 0.388 M…

A: Calcium hydroxide and perchloric acid undergo acid-base neutralization reaction. The balanced…

Q: what is the concentration of sodium chloride in the diluted solution?

A: Molarity = number of moles of solute/volume of solution (in L) so, moles = molarity × volume (in L)…

Q: What is the final concentration of the nitrate anion?

A: Number of moles = molarity × volume(in L) Final concentration of Nitrate anions = total moles of…

Q: You wish to make a 0.338 M hydrochloric acid solution from a stock solution of 12.0 M hydrochloric…

A: Concentrated solutions upon addition of water gets diluted to lower concentrations. The dilution of…

Q: What volume of a 0.173 M perchloric acid solution is required to neutralize 21.5 mL of a 0.162 M…

Q: You add 50. mL of water to 30. mL of a 0.50 M stock HCl solution. What is the [HCl] of the new,…

A: Given:: Initial, M1= 0.50 M , V1= 30. mL Final, M2= ? V2= (30+50)= 80 ml

Q: A 373-mL sample of a 0.481-M CaCl2 solution is left on a hot plate overnight; the following morning,…

A: The objective of this question is to find out the volume of water that evaporated from the CaCl2…

Q: If 52.00 ml of 0.500 M CaBr 2 solution is added to 128 ml of 0.320 M solution of KCl solution, what…

Q: A chemist has a 0.32 M stock solution. The chemist dilutes 18.1 mL of this solution into a 50.0 mL…

A: Given, Stock solution: Concentration of the stock solution (M1) = 0.32 M Volume of the stock…

Q: The normality of an aqueous solution of hydrobromic acid is determined by titration with a 0.151 N…

A: Given : N1 = 0.151 N , V1 = 32.8 mL V2= 16.7 mL Tip: N1V1 = N2V2

Q: In the laboratory a student combines 31.7 mL of a 0.167 M calcium nitrate solution with 20.9 mL of a…

A: Number of moles of calcium nitrate and ammonium nitrate can be calculated as follows:

Q: A 21.8 mL solution of 14.2 M HCl is diluted to 228 mL. What is the new concentration of the acid…

A: Given : Initial concentration of HCl = 14.2 M Initial volume of solution = 21.8 mL And final volume…

Q: 10.0 mL sample of an HCl solution is titrated with a 1.00 M NaOH solution. The neutralization…

A: Volume of HCl solution= 10 mL Molarity of NaOH= 1.0 M Volume of NaOH solution= 2.45 mL Molarity is…

Concept explainers

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.

Question

line teaching and lea X
+
om/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-... ☆
Visited
[Review Topics]
[References]
Use the References to access important values if needed for
this question.
In the laboratory a student combines 20.5 mL of a
0.177 M sodium phosphate solution with 12.7 mL of a
0.571 M sodium bromide solution.
What is the final concentration of sodium cation ?
M
Submit Answer
Retry Entire Group
9 more group attempts remaining
Previous
Next
I
Save and Exit
☐ X
S
11:09 PM
8/31/2022
...

Expert Solution

Step 1

Step by step

Solved in 2 steps with 2 images

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

M In the laboratory a student combines 23.6 mL of a 0.117 M aluminum bromide solution with 11.9 mL of a 0.353 M aluminum nitrate solution. M What is the final concentration of aluminum cation ? M
a 7.0 M HCl was mixed with 500 mL of 4.45 M HCl to attain a 5.65 M HCl solution, what volume of 5.65 M HCl can be made by the 2 mixtures?
An aqueous solution of sodium hydroxide is standardized by titration with a 0.109 M solution of nitric acid. If 14.6 mL of base are required to neutralize 15.2 mL of the acid, what is the molarity of the sodium hydroxide solution? M sodium hydroxide
In the laboratory, a student dilutes 22.3 of 6.05 M perchloric acid solution to a total volume of 300.0 mL. What is the concentration of the diluted solution?
In the laboratory you dilute 4.22 mL of a concentrated 6.00 M hydroiodic acid solution to a total volume of 100 mL. What is the concentration of the dilute solution? 3
You wish to make a 0.397 M nitric acid solution from a stock solution of 6.00 M nitric acid. How much concentrated acid must you add to obtain a total volume of 150 ml of the dilute solution? mL
we can precipitate out solid lead (II) iodide from an aqueous lead(II) nitrate solution by adding potassium iodide. if we have 500. mL of 0.632 M lead(II) nitrate solution how much 1.50 M potassium iodide must we add to exacltly precipitate all the lead (II) ions? 0.211 L 461 mL 0.632 L 0.421 L 0.316 L or 1.19 L
A 35.6 mL solution of 15.8 M HCl is diluted to 191 mL. What is the new concentration of the acid solution (in M)?
A2
An aqueous solution of hydroiodic acid is standardized by titration with a 0.108 M solution of barium hydroxide. If 21.8 mL of base are required to neutralize 17.8 mL of the acid, what is the molarity of the hydroiodic acid solution? M hydroiodic acid
What volume of a 0.313 M perchloric acid solution is required to neutralize 15.3 mL of a 0.185 M barium hydroxide solution? mL perchloric acid
In the laboratory a student combines 47.3 mL of a 0.247 M aluminum iodidesolution with 11.4 mL of a 0.431 M aluminum acetate solution. What is the final concentration of aluminum cation ?