4. Calculate the cation exchange capacity of the soil in which the following amounts of exchangeable cation are found. g/100g soil 0.0025 0.0152 Cation meq. wt. meq/100 g soil H K Са Mg NH, 0.3650 0.0920 0.0580

Determining the Ksp of Calcium Hydroxide Calcium hydroxide is an ionic solid that is sparingly soluble in water. A saturated, aqueous, solution of Ca(OH)2 is represented in equation form as shown below. Ca(OH)2 (s) → Ca²+ (aq) + 2OH(aq) The solubility product expression describes, in mathematical terms, the equilibrium that is established between the solid substance and its dissolved ions in an aqueous system. The equilibrium expression for calcium hydroxide is shown below. Ksp = [Ca²+][OH-]² The constant that illustrates a substance's solubility in water is called the Ksp. All compounds, even the highly soluble sodium chloride, have a Ksp. However, the Ksp of a compound is commonly considered only in cases where the compound is very slightly soluble and the amount of dissolved ions is not simple to measure. Your primary objective in this experiment is to test a saturated solution of calcium hydroxide and use your observations and measurements to calculate the Ksp of the compound. You…

Sodium nitrate contains 0.3% iodine in the form of calcium iodate, Ca(IO3)2. After the sodium nitrate in the niter is dissolved and recrystallized, the remaining solution contains 9 g/Lsodium iodate, NaIO3(aq). The NaIO3 is converted to iodine when it reactswith sulfur dioxide and water.2NaIO3 + 5SO2 + 4H2O → Na2SO4 + 4H2SO4 + I2a. How many liters of sodium iodate solution that contains 9 g of NaIO3 perliter would be necessary to form 127.23 kg of iodine, I2?

0.376 grams of KHP are placed in an Erlenmeyer flask and some water and a drop of phenolphthalein is added to the flask.  The buret is filled with an NaOH (aq) solution of unknown concentration.  The NaOH solution is added dropwise to the flask containing KHP (aq).  After 12.78 mLs of the NaOH(aq) solution is added, the color of the solution is found to be faintly pink. What is the concentration (M) of the unknown NaOH solution based on this data alone?

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2 (aq) + OH" (aq)NO, (aq) + H2O (1) K =

3.02 g of sodium sulfate was mixed into a solution containing 48.5 mL of 0.185 mol/L aqueous silver nitrate:   Calculate the maximum mass (in g) of precipitate that can form.   Note: Balanced chemical eq. with state of each compound required.       2. What is the molar concentration of sodium ions in the resulting solution?

The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)

Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H2O(1) =NH,* (aq) + OH(aq) K=-

Calculate the pOH of a 0.0376 M HCIO solution at each temperature. 0°C pOH = 35 °C pOH = T (°C) 0 5 10 15 20 30 35 40 45 50 100 Kw 1.15 x 10 1.88 x 10 2.97 x 10 4.57 x 10 6.88 x 10 1.46 × 10 2.07 x 10 2.88 x 10 3.94 x 10 5.31 x 10 5.43 x 10 45 45 44 H 45 15 15 14 +4 44

Consider the table of equilibrium constant values given below for a given set of conditions. What will be the concentration of [HCO3-] in water that is in equilibrium with both CaCO3 (s) and 225 ppm CO2 (g) under these conditions? Equation Type Value CO2 (g) H2CO3 (aq) KH 1.7 x 102 H2CO3 (aq)=HCO3(aq) + H (aq) Kat 6.44 x 107 HCO3 (aq) CO32 (aq) + H* (aq) Ka2 8.43 x 10-11 CaCO3 (s) Ca2+ (aq) + CO2 (aq) Ksp 8.4 x 10-9 H₂O (1) H(aq) + OH (aq) Kw 7.6 x 10-14 O 1.6 x 103 M O 8.1 x 10-3 M O 5.6 x 104 M O 3.9 x 104 M O 7.9 x 104 M