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5. How does the equilibrium constant...
please answer all parts of this question and explain everything 3. Give the simplest expression for determining the...
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3. Give the simplest expression for determining the equilibrium concentration of phosphate ions in a solution prepared with an analytical concentration of phosphoric acid of CH3PO4 and a given pH.
please answer all parts of this question and explain everything 5. Using HSAB theory, choose the...
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5. Using HSAB theory, choose the better acid or base in the following pairs and explain your choice: a. CH3NH2 or NH3 in reaction with H b. Which end of SCN will coordinate to Cr"; Pt?? c. Boric acid, B(OH)3, acts as an acid in water, but does not do so via ionization of a proton. Rather, it serves as a Lewis acid towards OH. Explain with the use of...
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2. Give the equation for calculating the fractional composition of phosphate, apo in an aqueous solution.
Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g)...
Be sure to answer all parts. At 1280°C the equilibrium constant Kc for the reaction Br2(g) ⇌ 2Br(g) is 1.1 × 10−3. If the initial concentrations are [Br2] = 0.0390 M and [Br] = 0.0370 M, calculate the concentrations of these two species at equilibrium. [Br2]eq [Br]eq
please answer all the parts Supplemental Questions - Titration Lab, 1. Indicate how each of the...
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Supplemental Questions - Titration Lab, 1. Indicate how each of the following would affect the values of K, for the weak acid unknown and for the dibasic salt and the value of the molar mass for the dibasic salt (Would the determined values be higher or lower than the actual values?). Use larger, smaller or no change. And as always....Explain. a. The titrant (either the NaOH or the HCI) molarity is actually HIGHER than that...
please answer all parts of this question and explain everything 3. For each of the following...
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3. For each of the following reactions, identify the acid and base. Also indicate which acid- base definition (Lewis, solvent system, Brønsted) applies. In some cases more than one definition may apply. a. 2 HF + SbFs 5 [H2F] + [SbF6] b. XeO; + OH = [XO H) c. PtFs + CIF3 = (CIF)* + [PtF6] d. 2 CH3Hg. + CaCl2 = Cal2 + 2 CH3HgCI e. [AgCl2] (aq) +...
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + Br2(g)...
Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr in a 18.1−L reaction vessel, calculate the concentrations of H2, Br2, and HBr at equilibrium. [H2] =___ M Br2] = ___M [HBr] = ____M
Be sure to answer all parts. The equilibrium constant Kc for the reaction I2(g) ⇆ 2I(g)...
Be sure to answer all parts. The equilibrium constant Kc for the reaction I2(g) ⇆ 2I(g) is 3.84 × 10−5 at 724 ° C. Calculate Kc and KP for the equilibrium 2I(g) ⇆ I2(g) at the same temperature. Kc = × 10 (Enter your answer in scientific notation.) KP =
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Dont't copy please answer all parts of this question and explain everything please. thank you 7) You isolate a mutant strain of mice that grow at an unusually fast rate, perform a blood test on the mice, and find that they have elevated levels of insulin-like growth factor2. The phenotype is the result of a mutation in a region of the genome containing a gene encoding a DNA methylase. What kind of mutation is causing the rapid growth of these...
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Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I2(g) - 21g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 × 10-5. Suppose you start with 0.0458 mol of I2 in a 2.33-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2? What is the equilibrium...
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3. Give the simplest expression for determining the equilibrium concentration of phosphate ions in a solution prepared with an analytical concentration of phosphoric acid of CH3PO4 and a given pH.
please answer all parts of this question and explain
everything
5. Using HSAB theory, choose the better acid or base in the following pairs and explain your choice: a. CH3NH2 or NH3 in reaction with H b. Which end of SCN will coordinate to Cr"; Pt?? c. Boric acid, B(OH)3, acts as an acid in water, but does not do so via ionization of a proton. Rather, it serves as a Lewis acid towards OH. Explain with the use of...
please answer all parts of this question and explain
everything
2. Give the equation for calculating the fractional composition of phosphate, apo in an aqueous solution.
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Supplemental Questions - Titration Lab, 1. Indicate how each of the following would affect the values of K, for the weak acid unknown and for the dibasic salt and the value of the molar mass for the dibasic salt (Would the determined values be higher or lower than the actual values?). Use larger, smaller or no change. And as always....Explain. a. The titrant (either the NaOH or the HCI) molarity is actually HIGHER than that...
please answer all parts of this question and explain
everything
3. For each of the following reactions, identify the acid and base. Also indicate which acid- base definition (Lewis, solvent system, Brønsted) applies. In some cases more than one definition may apply. a. 2 HF + SbFs 5 [H2F] + [SbF6] b. XeO; + OH = [XO H) c. PtFs + CIF3 = (CIF)* + [PtF6] d. 2 CH3Hg. + CaCl2 = Cal2 + 2 CH3HgCI e. [AgCl2] (aq) +...
Please help me with this question and help me understand
that.
Be sure to answer all parts. The dissociation of molecular iodine into iodine atoms is represented as I2(g) - 21g) At 1000 K, the equilibrium constant Kc for the reaction is 3.80 × 10-5. Suppose you start with 0.0458 mol of I2 in a 2.33-L flask at 1000 K. What are the concentrations of the gases at equilibrium? What is the equilibrium concentration of I2? What is the equilibrium...
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