B) Sample Problem: A chemist prepares a solution by dissolving .8 mole of NaOH in water to give a 50 ml solution. What is the molarity of this solution? (C) Sample problem: What is molality of a solution prepared by dissolving 20g MgCl2 in 250 g water? (D) Sample Problem: What is the mole fraction of the particles contained in a 25% sucrose ?

B) Sample Problem: A chemist prepares a solution by dissolving .8 mole of NaOH in water to give a 50 ml solution. What is the molarity of this solution? (C) Sample problem: What is molality of a solution prepared by dissolving 20g MgCl2 in 250 g water? (D) Sample Problem: What is the mole fraction of the particles contained in a 25% sucrose ?

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter16: Solutions

Section: Chapter Questions

Problem 16.3TC

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(A) Sample Problem: A 12.1 Moles NaOH solution means there are 12.1 moles of NaOH in liter of solution. Preparation of 12.1 M NaOH: Step 2: Now weigh -___of NaOH (resulted mass of NaOH in step 1) using balance.
What is the concentration in units of grams of dye per liter of solution ,of the dilute dye solution that is produced as follows? transfer 19.53 ml of stick solution (6.10g/L) to a 200.0Ml volumetric flask and dilute to the 200 ml line with deionized water. Correct number of significant figs
(b) (i) Based on the data given in TABLE 1, construct an energy cycle diagram for dissolution of lithium chloride, LiCl. TABLE 1 Process Enthalpy of reaction (kJ mol-) Lattice energy of LiCl AH = - 846 Dissolution of LiCl AH = - 77 Hydration of Li* Hydration of CF AH = - 510 AH = - 413 (ii) Which of these salts, LiCl or KCl, would have larger lattice energy? Explain.
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A supersaturated solution of sucrose (C12H22O11) is madeby dissolving sucrose in hot water and slowly letting thesolution cool to room temperature. After a long time, theexcess sucrose crystallizes out of the solution. Indicatewhether each of the following statements is true or false:(a) After the excess sucrose has crystallized out, the remainingsolution is saturated.(b) After the excess sucrose has crystallized out, the systemis now unstable and is not in equilibrium.(c) After the excess sucrose has crystallized out, the rate ofsucrose molecules leaving the surface of the crystals tobe hydrated by water is equal to the rate of sucrose moleculesin water attaching to the surface of the crystals.
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Now let's use this information to solve a problem: An unknown amount of barium nitrate is dissolved in 120.0 g of water and 8.15 g of copper (I) sulfate Is dissolved in 75.0g of water. When these solutions are mixed 1.076g of white solid is isolated as a precipitate by vácuum filtration, The filtrate is found to have a mass of 204.44 g. What mass of barlum nitrate was dissolved in the water and used for this reaction? mass of barium nitrate =
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An aqueous solution of sucrose (C12H22O11) is prepared by dissolving 7.4045 g in sufficient deionized water to form a 100.00 mL solution. Calculate the molarity of the solution. Do you mind showing work? I would assume that (given) gram weight (times moles present/divided by mole(s) of compound) then divided - again by compound weight will give a percentage, then divded by the .....that's where I'm a little lost. thanks
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