Answered: What is the freezing point of 8.0 ×…

What is the freezing point of 8.0 × 10-8 m aqueous sodium phosphate, Na3PO4? Use the formula of the salt to obtain i. K;(water) = 1.858°C/m Freezing point = °C

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

Similar questions

A student determined the average molarity of their sample of acetic acid to be 0.611 M. Calculate the (w/w)% of the solution. Assume the density of this solution is that of pure water, dH2O = 1000. g/L. Enter a number without the '%' symbol.
The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of chromium(II) nitrate (176.0 g/mol), must be dissolved in 295.0 grams of water to reduce the freezing point by 0.450 °C? Refer to the table for the necessary boiling or freezing point constant. Formula Kb (°C/m) Kf(°C/m) H₂O 0.512 CH3 CH₂ OH 1.22 CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH₂ CH3 2.02 Solvent Water Ethanol Chloroform Mass= g 1.86 1.99 5.12
Complete combustion of 8.653 g of a compound of carbon, hydrogen, and oxygen yielded 21.83 g CO₂ and 3.831 g H₂O. When 18.00 g of the compound was dissolved in 288 g of water, the freezing point of the solution was found to be -0.952 °C. For water, Kfp = = 1.86 °C/m. What is the molecular formula of the compound? Enter the elements in the order C, H, O molecular formula =
A student determined the average molarity of their sample of acetic acid to be 0.536 M. Calculate the (w/w)% of the solution. Assume the density of this solution is that of pure water, dH2O = 1000. g/L. Enter a number without the '%' symbol. (I'm struggling to find the Volume from the attached equation(s) that are "meant" to be used for this problem)
The solution is in steps on paper
The freezing point of water is 0.00°C at 1 atmosphere. How many grams of chromium(III) nitrate (238.0 g/mol), must be dissolved in 255.0 grams of water to reduce the freezing point by 0.450°C ? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 x Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 x _________g chromium(III) nitrate.
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of cobalt(II) chloride (129.8 g/mol), must be dissolved in 250.0 grams of water to raise the boiling point by 0.450°C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf (°C/m) Water H20 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHC13 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g cobalt(II) chloride.
A certain liquid X has a normal boiling point of 92.90°C and a boiling point elevation constant Kb=2.15·°C·kgmol−1. Calculate the boiling point of a solution made of 30.g of potassium bromide (KBr) dissolved in 800.g of X. Round your answer to 3 significant digits.
The boiling point of water is 100.0°C at 1 atmosphere. How many grams of potassium iodide (166.0 g/mol), must be dissolved in 242.0 grams of water to raise the boiling point by 0.500 °C? Refer to the table for the necessary boiling or freezing point constant. Kb(°C/m) Kƒ(°C/m) Solvent Formula Mass = H₂O CH3 CH₂OH Water 0.512 Ethanol 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH2 CH3 2.02 g potassium iodide 1.86 1.99 5.12
A copper(II) sulfate solution is 14.0% CuSO4 by mass. It is simultaneously 1.01 M at 20 °C. (a) Compute the density of this solution. Density= 8 cm-3 (b) What volume of this solution should be used in preparing 1.44 L of a 9.60×10-² M copper(II) sulfate solution? Volume mL