Learning Activity Worksheets GRADE 6- Science
True or false
8.The combination of a solid and a liquid substance will depend on the ability of the liquid to dissolve the solid, or the capacity of the solid to be dissolved in the liquid.
9. A mixture can come in any form. It may be solid, liquid, or in gaseous form.
10. Air is a mixture of different kind of gases.
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True or false
8.The combination of a solid and a liquid substance will depend on the ability of the liquid to dissolve the solid, or the capacity of the solid to be dissolved in the liquid.
9. A mixture can come in any form. It may be solid, liquid, or in gaseous form.
10. Air is a mixture of different kind of gases.
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8.The combination of a solid and a liquid substance will depend on the ability of the liquid to dissolve the solid, or the capacity of the solid to be dissolved in the liquid.
True
9. A mixture can come in any form. It may be solid, liquid, or in gaseous form.
false
10. Air is a mixture of different kind of gases.
true
Explanation:
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me 2 grade 6 science
[tex]\huge\tt\green{{EXPLANATION:}}[/tex][tex]\large\bold\blue{{Factos \: Affecting \: Solubility}}[/tex]
➤ The Maximum amount of a solute that can dissolve in a solvent at a specified temperature and pressure is its Solubility. Solubility is often expressed as the mass of solute per Volume (g/L) or mass of solute per mass of solvent (g/g), or as the moles of solute per Volume (mol/L). Even for very soluble Substances, However, There is usually a limit to how much solute can dissolve in a given Quantity of Solvent. In General, The Solubility of as Substance depends on not only the energetic factors we have discussed but also the temperature and, for gases, the pressure. At 20°C, for example, 177 g of NaI, 91.2 g of NaBr, 35.9 g of NaCl, and only 4.1 g of NaF dissolve in 100 g of water. At 70°C, however, the solubilities increase to 295 g of NaI, 119 g of NaBr, 37.5 g of NaCl, and 4.8 g of NaF. As you learned in Chapter 12, the lattice energies of the sodium halides increase from NaI to NaF. The fact that the solubilities decrease as the lattice energy increases suggests that the [tex]ΔH2[/tex] term in Figure 13.1 dominates for this series of compounds.
[tex]\\[/tex]
[tex]\small\bold\blue{{The \: Solubility \: of \: most \: solids \: increases \: with}}[/tex][tex]\small\bold\blue{{increasing \: temperature.}}[/tex]
➤ Because the Solubility of most solids increases with increasing temperature, a Saturated solution that was prepared at a higher temperature usually contains more dissolved solute than it would contain at a lower temperature. When the solution is cooled, it can therefore become supersaturated (Figure 13.2.1c ). Like a supercooled or Superheated Liquid, a supersaturated solution is unstable. Consequently, adding a small particle of the solute, A Seed Crystal, will usually cause the excess solute to rapidly Precipitate or crystallize, sometimes with spectacular results. The rate of Crystallization in Equation is greater than the rate of dissolution, so crystals or a Precipitate form (Figure 13.2.1d ). In contrast, adding a Seed Crystal to a Saturated solution reestablishes the dynamic Equilibrium, and the net quantity of dissolved solute no longer changes.