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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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calculate the boiling point elevation and freezing point depression of 3.om solution in sucrose of water. The K\/b for water is 0.512 degrees C/m and the K\/f for water is 1.86 degrees C/m.
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- Pleae keep in mind sig figs and if it needs scientific notation. TYSM :)arrow_forwardP. The normal boiling point of a certain liquid X is 142.70 °C, but when 0.13 kg of barium hydroxide (Ba(OH),) are dissolved in 750. g of X the solution boils at 144.4°C instead. Use this information to calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. °C-kg OLX = 'x Continue Submit Assignment O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility EPIC MacBook Pro F3 F8 F10 #3 3. $ 8 R. T. A H と alt pubuwo command optionarrow_forwardA certain liquid x has a normal freezing point of 1.30 °C and a freezing point depression constant K,- 3.30 °C-kg'mol!. A solution is prepared by dissolving some glycine (c,H,NO,) in 850. g of x. This solution freezes at - 2.2 °C. Calculate the mass of c,H,NO, that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. ?arrow_forward
- Ethanol has a Kb of 1.22 oC/m and usually boils at 78.4 oC. This means that the boiling point elevation for ethanol is give by the equation: BPE = 1.22 MT where MT is the total number of moles of solute particles per liter of solution How many moles of an nonionizing solute would need to be added to 47.32 mL of ethanol in order to raise the boiling point to 87.1 oC.arrow_forwardName Time M T W R F The freezing point of pure benzene (CH,) is 5.50°C. The freezing point of a solution containing 5.00 g of an unknown non-dissociating solute in 444 g of benzene is 5.07°C. K, of benzene = 4.90°C/m. Show complete calculations for each question below. 1. What is the freezing point depression for this solution?arrow_forwardAn experiment was conducted to determine the effect of glucose on the freezing point of water. Experimental data showed thatthe freezing point depression of water in solution was –2.6°C when 1.0 g of glucose was dissolved in 10g of solvent. Calculatethe expected freezing point for such solution and compare the expected freezing point to the value found experimentally. Give aplausible explanation for any discrepancies. (M.W. of glucose= 180.16g/mol; i=1). Show all your work.arrow_forward
- From your data in Part 1 of the experiment, you calculate the natural log of the partial pressure of water and 1/T value in K for 5 points between 50°C and 80°C. You make a graph of In(P) vs. 1/T and determine that the slope of the linear line is -4800 K. Use this information to calculate AHvap of water. Make sure to use R = 8.314 J mol-1-K-1. Oa. 46.6 kJ/mol Ob. 0.578 kJ/mol Oc. 31.5 kJ/mol O d. 39.9 kJ/molarrow_forwardConsider a solution of 0.877 molal (m) ethanol in water. Considering the normal boiling point for water is 100 °C, and the boiling pont elevation constant for water is 0.51 °C/m, what is the boiling point of this mixure? Report anser two places past the decimal point.arrow_forward||| O STATES OF MATTER Using the Kf and Kb equations with electrolytes A certain liquid X has a normal freezing point of 3.50 °C and a freezing point depression constant K, -5.23 °C-kg-mol solution made of 39.g of zinc chloride (ZnCl₂) dissolved in 450. g of X. Round your answer to 1 significant digit. *c X ODD Calculate the freezing point of aarrow_forward
- When 127. mg of a certain molecular compound X are dissolved in 55.0 g of dibenzyl ether point of the solution is measured to be 1.6 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. ((C6H₂CH₂)₂0), 2 the freezing OO B olo Xuarrow_forward"hen 142. g of alanine (C3H,NO2) : are dissolved in 1500. g of a certain mystery liquid X, the freezing point of the solution is 7.30 °C less than the freezing pint of pure X. (Fe(NO:),)* alculate the mass of iron(III) nitrate that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't off factor i=3.80 for iron(III) nitrate in X. e sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.arrow_forwardCalculate the molal freezing point depression constant of Kf of X.arrow_forward
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