Suppose 0.177 g of iron(II) bromide is dissolved in 50. mL of a 52.0 m M aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the iron(II) bromide is dissolved in it. Be sure your answer has the correct number of significant digits. M X S ale A !!

Suppose 0.177 g of iron(II) bromide is dissolved in 50. mL of a 52.0 m M aqueous solution of silver nitrate. Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the iron(II) bromide is dissolved in it. Be sure your answer has the correct number of significant digits. M X S ale A !!

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 38CR

See similar textbooks

Related questions

Q: A chemistry student must write down in her lab notebook the concentration of a solution of sodium…

Q: Suppose 0.317 g of barium acetate is dissolved in 50. mL of a 80.0 m M aqueous solution of ammonium…

A: Mass of barium acetate =0.317 gVolume of ammonium sulfate = 50 mL = Molarity of ammonium sulfate =…

Q: A 25.0 ml solution of 0.500 M NaOH is titrated until neutralized into a 35.0 ml sample of HCl. What…

A: In this problem, we are dealing with a titration of sodium hydroxide (NaOH) into hydrochloric acid…

Q: A chemist prepares a solution of aluminum chloride (AICI,) by measuring out 49.6 umol of aluminum…

A: We have to express the concentration in mmol/L. It is given that 49.6 micromoles of AlC3 is used, So…

Q: A chemist prepares a solution of iron (II) bromide (FeBr₂) by measuring out 8.06 mg of FeBr₂ into a…

A: To calculate the molarity of Br- anions in the solution, we need to determine the number of moles of…

Q: Suppose 23.8 g of sodium iodide is dissolved in 350. mL of a 0.80 M aqueous solution of silver…

Q: Suppose 11.1g of lead(II) acetate is dissolved in 350.mL of a 0.80 M aqueous solution of…

A: Given that : The mass of lead (II) acetate = 11.1 g The volume of ammonium sulfate solution = 350 mL…

Q: when doing a test to find the molarity of solution of hydrochloric acid, the following results were…

A: Accuracy: Accuracy refers to how closely the measured value of the quantity corresponds to its…

Q: A sample of MgCl,(5) is added to water and the number of chloride ions is measured to be 8 x 10.…

A: Given: Number of chloride ions = 8 × 1022 ions. And volume of solution = 5.0 L

Q: Suppose 37.3 g of ammonium iodide is dissolved in 300. mL of a 0.60 M aqueous solution of potassium…

A: We have to calculate molarity of iodide anion

Q: A chemistry student must write down in her lab notebook the concentration of a solution of sodium…

Q: An analytical chemist weighs out 0.061 g of an unknown monoprotic acid into a 250 mL volumetric…

A: Given: Mass of acid = 0.061 g Molarity of NaOH = 0.1900 M Volume of NaOH = 3.3 mL = 0.0033 L

Q: Suppose 0.413 g of copper(II) nitrate is dissolved in 150. mL of a 17.0 m M aqueous solution of…

A: Let's consider that the volume of the solution does not change after dissolving copper(II) nitrate.…

Question

Suppose 0.177 g of iron(II) bromide is dissolved in 50. mL of a 52.0 m M aqueous solution of silver nitrate.
Calculate the final molarity of bromide anion in the solution. You can assume the volume of the solution doesn't change when the iron(II) bromide is dissolved in
it.
Be sure your answer has the correct number of significant digits.
M
Explanation
Check
X
3
MacBook Air
ala
14
Ar
99
© 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessi

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: Number of moles of iron bromide and silver nitrate

VIEW

Step 2: Reaction between iron bromide and silver nitrate

VIEW

Solution

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 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

What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
35. For each of the following solutions, the mass of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 3.51 g NaCl: 25 mL c. 3.51 g NaCl: 75 mL b. 3.51 g NaCl; 50. mL d. 3.51 g NaCl; l.00 L
A student wants to prepare 1.00 L of a 1.00-M solution of NaOH (molar mass = 40.00 g/mol). If solid NaOH is available, how would the student prepare this solution? If 2.00 M NaOH is available, how would the student prepare the solution? To help ensure three significant figures in the NaOH molarity, to how many significant figures should the volumes and mass be determined?
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?
Without consulting your textbook, list and explain the main postulates of the kinetic molecular theory for gases. How do these postulates help us account for the following bulk properties of a gas: the pressure of the gas and why the pressure of the gas increases with increased temperature; the fact that a gas tills its entire container; and the fact that the volume of a given sample of gas increases as its temperature is increased.
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.
A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
ou have two solutions containing solute A. To determine which solution has the highest concentration of A in molarity, which of the following must you know? (There may be more than one answer.) the mass in grams of A in each solution the molar mass of A the volume of’ water added to each solution the total volume of the solution plain your answer.
A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O