4. Figure 16.3 shows the solubility of AgNO, in water in units of moles of AgNO, per kilogram of H;O. If 255 g of AGNO, is added to 100 g of water at 95°C and cooled slowly, at what temperature will the solution become saturated? FIGURE 16.3 Most solubilities increase with increasing temperature, but some decrease. Note that the 25 changes are not always smooth because different solid hydrates form over different temperature ranges. AGNO3 20 AgF 15 10 NaCH;COO NaCl NANO3 KCIO4 0.3 0.2 Cez(SO4)3 0.1 CaSO4 0.0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Solubility (moles of solute per kg of water)

4. Figure 16.3 shows the solubility of AgNO, in water in units of moles of AgNO, per kilogram of H;O. If 255 g of AGNO, is added to 100 g of water at 95°C and cooled slowly, at what temperature will the solution become saturated? FIGURE 16.3 Most solubilities increase with increasing temperature, but some decrease. Note that the 25 changes are not always smooth because different solid hydrates form over different temperature ranges. AGNO3 20 AgF 15 10 NaCH;COO NaCl NANO3 KCIO4 0.3 0.2 Cez(SO4)3 0.1 CaSO4 0.0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Solubility (moles of solute per kg of water)

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

Tiny samples of aqueous solutions are sketched below, as if under a microscope so powerful that individual molecules could be seen. (The water molecules are not shown.) The two substances in each sample can interconvert. That is, each kind of molecule can turn into the other. The equilibrium constant K for each interconversion equilibrium is shown below the sketch. Decide whether each solution is at equilibrium. Coo yes 000 8 At equilibrium? yes 1 K = = = = 8 9 no K=9 At equilibrium? O no At equilibrium? O yes K= 4 yes no 3 K= 2 At equilibrium? no X
Suppose a 250. mL flask is filled with 1.5 mol of CO, 0.30 mol of H,O and 1.3 mol of H,. The following reaction becomes possible: CO(g) +H,0(g)– CO2(g)+H,(g) The equilibrium constant K for this reaction is 1.25 at the temperature of the flask. Calculate the equilibrium molarity of H,O. Round your answer to two decimal places. OM
PCI5(g) → PCI3(g) + Cl2(g) has K, = 1.84 at a given temperature. What is the value of K, for the reaction PCI3(g) + Cl2(g)PCI5(g) at the same temperature? %3D 1.84
At 70 °C, the solubility of an unknown solute is 65.7 g/100.0 g of water. What mass of the solute can dissolve in 125.5 g of water at the same temperature?
The solubility limit of a solute at 20. °C and 1.0 atm is 13.8 g of solute per 1 L of water. What will MOST likely happen when 12.0 g of solute are added to 1 L of pure water and the solution is mixed well (at the same conditions)?
Predicting the products of dissolution The names and chemical formulae of some chemical compounds are written in the first two columns 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. Then, write down in the third column of the table the chemical formula of the major chemical species that will be present in this solution. For example, you know water itself will be present, so you can begin each list with the chemical formula for water (H₂O). 6 Note: "major" chemical species are those present in concentrations greater than 10 compound potassium cyanide copper(II) iodide sucrose formula KCN Cul₂ C12H₂2O11 major species present when dissolved in water 0 0 0 × mol/L. On 3/5 0,0,... S ? allo 18 Ar
The CO2 gas sealed inside a carbonated beverage bottle has a pressure of 1.9atm. At this pressure, the solubility of CO, in water is 0.065g CO2/100 g H20. When the bottle is opened,the CO2 in the space above the liquid escapes, and the partial pressure of the CO2 falls to 2.3 mmHg, the value in the surrounding atmosphere of the room. Calculate the solubility of CO2 in the beverage at this new pressure, assuming no changes in temperature occur. Give the result in 2 sig. figs. 2.6 x 10^ -4 g of CO2 in 100 g of water.
At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what is the solubility of oxygen in water exposed to air at 1.00 atm? solubility: At 298 K, what is the solubility of oxygen in water exposed to air at 0.900 atm? solubility: If atmospheric pressure suddenly changes from 1.00 atm to 0.900 atm at 298 K, how much oxygen will be released from 4.80 L of water in an unsealed container? amount: MacBook Pro Search or type URL + M M mol
At a certain temperature, a saturated solution contains 557 g NaOH(s) per liter of solution. Calculate the molarity of this saturated NaOH(aq) solution. please explain how to reach the molarity?
Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing point depression constant for water is Kf = 1.86 C/kg Use the table provided to answer the question. 1.00 g of Lead (II) Sulfate is mixed into 5.75 L of water. a) How many moles of the Lead (III) Sulfate will actually dissolve into the water? b) How many grams of Lead (III) Sulfate will be left un-dissolved? c) At what temperature will the solution now boil and freeze?
A 1.35 m aqueous solution of Compound X had a boiling point of 102.8°C. Which one of the following is most likely to be Compound X? Hint: The boiling point elevation constant for water is 0.52°C/m. Na3PO4 CaCl₂ X OKCI CH3CH₂OH
Predicting the products of dissolution The names and chemical formulae of some chemical compounds are written in the first two columns 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. Then, write down in the third column of the table the chemical formula of the major chemical species that will be present in this solution. For example, you know water itself will be present, so you can begin each list with the chemical formula for water (H,O). -6 mol/L. Note: "major" chemical species are those present in concentrations greater than 10 dlo major species present when dissolved in water compound formula ammonium bromide NH,Br propylene glycol C;H,(OH), glycerol C;H,O; 11:53 AM 4/19/2021 P Type here to search