Using the Kf and Kb equations with electrolytes. - 1A solution is prepared by9.A certain liquid X has a normal boiling point of 144.20 °C and a boiling point elevation constant K,=0.76 °C·kg•moldissolving some ammonium chloride (NH,Cl) in 150. g of X. This solution boils at 145.3 °C. Calculate the mass of NH,Cl that was dissolved.Be sure your answer is rounded to the correct number of significiant digits.x10

Boiling point of solution = 145.3 °c Boiling point of solvent = 144.2 °c □Tb = 145.3 - 145.2 =…

liquid X has a normal boiling point of 144.20 °C and a boiling point elevation constant K,=0.76 °C·kg•mol g some ammonium chloride (NH,Cl) in 150. g of X. This solution boils at 145.3 °C. Calculate the mass of NH,C your answer is rounded to the correct number of significiant digits.

liquid X has a normal boiling point of 144.20 °C and a boiling point elevation constant K,=0.76 °C·kg•mol g some ammonium chloride (NH,Cl) in 150. g of X. This solution boils at 145.3 °C. Calculate the mass of NH,C your answer is rounded to the correct number of significiant digits.

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 buffer solution is made that is 0.385 M in HNO2 and 0.385 M in KNO2. If Ka for HNO2 is 4.50 x 10,…

A: We have to find the pH

Q: the value of Ksp for Cu(1O,),.

Q: Calculate the molar solubility of AgCl in a 3.00 L solution containing 14.0 g of dissolved CaCl,.…

Q: please skip this if you have already answered. I will only upvote if it is complete and correct.…

A: We have asked to complete each of the given statements correctly, And the correct statements are…

Q: What is the Molar Mass (g/mol) of an unknown monoprotic weak acid if 648 mg of it requires 35.86 mL…

Q: Why is there a need for buffers? Please explain in depth and detail

A: A buffer solution is a solution that can withstand changes in pH on addition of acidic or basic…

Q: When 22.0 mL of a 3.34×10M sodium carbonate solution is combined with 15.0 mL of a 1.06×10“ M lead…

A: Given data for part a)Molarity of Na2CO3=3.34×10-4MVolume of Na2CO3=22.0mL=0.022LMolarity of…

Q: Are salts soluble in liquid ammonia?

A: Liquid ammonia is a good solvent for organic compounds But it is a worse solvent for inorganic…

Q: What would happen to the ratio?

A: PH of a solution = - log [H+] From the relation we can say that pH of solution is inversely…

Q: Please don't provide handwritten solution ....

A: The number of moles of NaOH:moles of NaOH=molarity of NaOH×volume of the solution in L=0.242…

Q: Acetic acid buffers are most effective in resisting pH changes to

A: a solution which resist in ph change value upon adiition of small amount of strong acid or base…

Q: What equation is used in calculating the pH of buffers? What expression does this equation derive…

A: Buffer Solution is a water-based solution that consists of a mixture of a weak acid and its…

Q: 2. What is the pH of the buffer system after the ad of the solution gaseous HCl to 1

A: The solutions which resists its pH by addition of small aamount of strong acid (or) strong base…

Q: A solution is made by adding HCN to yield a concentration of 0.01 M and KCN to yield a concentration…

A: The quantitative method to determine the acidity or basic strength of a medium is to determine pH.…

Q: The molar solubility of silver sulfide in a water solution is M.

A: We know according to solubility rule most of sulfide are insoluble in water. So solubility product…

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

100%

Using the Kf and Kb equations with electrolytes.

- 1
A solution is prepared by
9.
A certain liquid X has a normal boiling point of 144.20 °C and a boiling point elevation constant K,=0.76 °C·kg•mol
dissolving some ammonium chloride (NH,Cl) in 150. g of X. This solution boils at 145.3 °C. Calculate the mass of NH,Cl that was dissolved.
Be sure your answer is rounded to the correct number of significiant digits.
x10

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

Beakers (a), (b), and (c) are representations of tiny sections (not to scale) of mixtures made from pure benzene and pure water. Select which beaker gives proper representation of the result when the two pure substances are mixed.
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.
solution is a homogeneous mixture. Can you give an example of a gaseous homogeneous mixture? A liquid homogeneous mixture? A solid homogeneous 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.
You want to prepare a 1.0 mol/kg solution of ethyleneglycol, C2H4(OH)2, in water. Calculate the mass of ethylene glycol you would need to mix with 950. g water.
Potassium sulfate has a solubility of 15 g/ 100 g water at 40C. A solution is prepared by adding 39.0 g of potassium sulfate to 225 g of water, carefully heating the solution, and cooling it to 40C. A homogeneous solution is obtained. Is this solution saturated, unsaturated, or supersaturated? The beaker is shaken, and precipitation occurs. How many grams of potassium sulfate would you expect to crystallize out?
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.
What is the difference between (a) mass and density? (b) an extensive and an intensive property? (c) a solvent and a solution?
1 A certain liquid X has a normal boiling point of 144.80 °C and a boiling point elevation constant K,=2.39 °C•kg•mol A solution is prepared by dissolving some glycine (C,H,NO,) in 650. g of X. This solution boils at 148.5 °C. Calculate the mass of C,H,NO, that was dissolved. Round your answer to 2 significant digits. olo Ar
A certain liquid X has a normal boiling point of 104.90 °C and a boiling point elevation constant K₁ = 0.61 °C-kg-mol prepared by dissolving some iron(II) nitrate (Fe(NO3)2) in 250. g of X. This solution boils at 105.6 °C. Calculate the mass of Fe(NO3), that was dissolved. Round your answer to 1 significant digit. g X 1 A solution is ? olo Ar
A certain liquid X has a normal boiling point of 129.30°C and a boiling point elevation constant =Kb2.32·°C·kgmol−1. A solution is prepared by dissolving some barium hydroxide (BaOH2) in 800.g of X. This solution boils at 130.2°C. Calculate the mass of BaOH2 that was dissolved. Round your answer to 1 significant digit. g
A certain liquid X has a normal boiling point of 147.30°C and a boiling point elevation constant =Kb2.24·°C·kgmol−1. Calculate the boiling point of a solution made of 14.0g of sodium chloride (NaCl) dissolved in 750.g of X.Round your answer to 5 significant digits. (Please dont round calculations untill the end.) °C