A student dissolves 10. g of phenol (C,H;OH) in 175. mL of a solvent with a density of 1.03 g/mL. The student notices that the volume of the solvent does not change when the phenol dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. do molarity = Ar molality =

The solubility of heptanol, CH3(CH₂)6OH, is 0.16 g per 0.10 L. What is the molarity of the solution? 0.073 0.013 0.0073 0.133 0.16

An aqueous solution of ethanol (molar mass = 46.07 g/mol) has a molality of 12.15 m and a density of 1.100 g/mL. What is the molarity of ethanol in the solution?

You are washing glassware in a lab. The solution your 1 L beaker contains 5 mol/L NaOH in water. It is known that 1% of the mixture adheres to the walls of the beaker when the beaker is drained. Thus, if you drain the beaker, 0.01 L of the original contents of the beaker remains in the beaker. The beaker must be filled with 1 L of pure water between each rinse. The beaker is then stirred very well.  What is the composition of the contents of the beaker, in mol/L, if it is rinsed once?  How many rinses does it take to get the contents of the beaker to below 0.00005 mol/L?

Use the solubility curve below to answer the following questions: 150 140 130 120 110 100 NANO3 90 80 70 60 NH&Cl KCI NaCi 50 40 30 20 KCIO3 10 Ce2(SOals O 10 20 30 40 50 60 70 80 90 100 Temperature (c) Q1) As the temperature increases, the solubility of the NH3 in water Q2) The solute, NH3, is MOST likely a (increases/decreases/stays the same). (solid, liquid, or gas). Q3) How many grams of NH4CI are dissolved in 500 g of water at 90 °C? Q4) If you had 50 grams of NH4CI in 100 g of water at 40 °C, would the solution be saturated, unsaturated, or supersaturated? Q5) You heat a solution of KCIO3 to 80°C and saturate the solution. You then allow the solution to cool down to 50°C. How many grams of solute would precipitate out of the solution? NH3 per 100 g H,0 Grams of solute ONO CON

Determine the freezing point (in °C) of a solution that contains 204 g of C6H1206 dissolved in 234 mL of acetic acid (density = 1.05 g/mL). Pure acetic acid has a freezing point of 16.6°C and a K = 3.90°C/m.

My X OWL X CICh x Para X EA ve X nment/takeCovalent Activity.do?locator=assignment-take uiz 5.pdf Solubility of Ionic Compounds Classify each of the compounds as soluble or not soluble: Miron (III) hydroxide cobalt(II) bromide magnesium iodide Submit Answer TREMENTS OCT W Math 122 Quiz 5.docx 12 tv (41 X [Review Topics] [References] Use the References to access important values if needed Retry Entire Group 9 more group attempts remaining PR F22-Chem-103x....pdf 2 Mic x A ΕΟ S Fel-F22-Ch

g at 10. °C. Calculate the volume of a saturated solution of X in water that mL The solubility in water of ionic compound X is measured and found to be 0.339 would contain 360. mg of X at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits.

Some chemical compounds are listed in the first column of the table below. Each compound is soluble in water.  imagine that a few tenths of a mole of each compound is dissolved in a liter of water. The important chemical species that would be present in the solution are written in the second column of the table. Use the checkboxes to classify each compound. 

Which of the following phrases best describes the term solubility?             the ability of a solvent to dissolve in a solute       the ability of a solute to dissolve in a solvent       the maximum amount of solute that will dissolve in solvent at a given temperature       the maximum amount of solvent that will dissolve in a solute at a given temperature       the amount of solvent that dissolves in a solute for each 10oC rise in temperature