Consider the solubilities of a particular solute at two different temperatures. Temperature ('C) Solubility (g/100 g H,0O) 20.0 41.3 30.0 71.3 Suppose a saturated solution of this solute was made using 77.0 g H,O at 20.0 °C. How much more solute can be added if the temperature is increased to 30.0 °C? mass: TOOLS x10

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

The solubility of a compound is 84 g per 100.0 g solvent at 25 °C. If 84 g of the compound is dissolved in 200.0 g of solvent at 25 °C, the solution is dilute unsaturated saturated supersaturated

A salt has a molar solubility of 4.18 M at 21.0°C. What is the the maximum amount of salt (in moles) that can dissolve in 1.495 L of solution before the solution becomes supersaturated at 21.0°C? Assume the salt has a molar mass of 55.44 g/mol. Report your answer to 2 decimal places.

What is the mole fraction of solute in a 3.12 m aqueous solution? Xsolute = x10 TOOLS

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In the blanks in the question, you have to decide if its increaseing or decreasing.

A solid mixture consists of 25.5 g of KNO3 (potassium nitrate) and 4.5 g of K₂SO4 (potassium sulfate). The mixture is added to 130. g of water. Use this solubility curve (Figure 1) to answer the Part C If the solution described in the introduction is cooled to 0 °C what mass of K2SO4 will crystallize?

An aqueous solution of isopropanol (MM = 60.10 g/mol) has a molality of 7.91 m and a density of 1.18 g/mL. What is the molarity of isopropanol in the solution?

What is the mole fraction of solute in a 3.69 m aqueous solution? Xsolute = x10 TOOLS