1. Which of the following compounds would be soluble or insoluble? (3 pts)KCIHg2Cl2(NH4)2CO3SolubleCr(NO3)6CaSO4PbCl2Insoluble2. Predict the products and circle P if the reaction is a precipitation or NR for no reaction.(1.5 pts)Sodium carbonate and copper (II) sulfate react to form what products?PNR3. Balance the following reaction: (1 pts)C10H22(g) +O2(l) →_CO2(aq) +H2O(g)4. How many grams of oxygen are present in 0.245 g of potassium sorbate (KC6H7O2)? (2pts)5. a. Oxygen-15 is a positron emitter. Write a balanced nuclear equation for the loss of apositron. (1.5 pts)b. Oxygen-15 is a beta (negatron) emitter. Write a balanced nuclear equation for the loss ofa negatron.b. Oxygen-15 is an alpha emitter. Write a balanced nuclear equation for the loss of an alphaparticle.

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Answered: 1. Which of the following compounds…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter20: Environmental Chemistry-earth's Environment, Energy, And Sustainability

Section: Chapter Questions

Problem 41PS

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5) The solubility of BaCO3 is 24 mg/L at room temperature. a. What is the molar solubility and the Ksp of barium carbonate? b. The carbonate ion can react with water as follows: CO3² (aq) + H₂O (1) HCO3 (aq) + OH- (aq) Kb = 2.1 x 10-4 Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined reaction. C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the solubility increase or decrease from part a? Explain using Le Chatelier's Principle.
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Experiment4: Solubility Product In the experiment to determine the solubility of KI04, in water, the following observations are made at a certain temperature: Volume of saturated KI04 solution taken in the conical flask = 25.0 mL KI added=2g H2SO4 (3.0 M ) added = 20.0 mL. Volume of 0.200M sodium thiosulphate used for titration = 8.00 mL Q1.If the mean ionic activity coefficient, γ± of KIO4 in the saturated solution is 0.85, what is Ksp of KIO4.?
Over time, as their free fatty acid (FFA) content increases,edible fats and oils become rancid. To measure rancidity, the fator oil is dissolved in ethanol, and any FFA present is titrated withKOH dissolved in ethanol. In a series of tests on olive oil, a stocksolution of 0.050 Methanolic KOH was prepared at 25C, storedat 0C, and then placed in a 100-mL buret to titrate any oleic acid[CH₃(CH₂)₇CH=CH(CH₂)₇COOH] present in the oil. Each offour 10.00-g samples of oil took several minutes to titrate: thefirst required 19.60 mL, the second 19.80 mL, and the third and fourth 20.00 mL of the ethanolic KOH.(a) What is the apparent acidity of each sample, in terms of mass% of oleic acid? (Note:As the ethanolic KOH warms in the bu-ret, its volume increases by a factor of 0.00104/C.)(b) Is the variation in acidity a random or systematic error? Ex-plain.(c) What is the actual acidity? How would you demonstrate this?
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VIII. A primary standard of HCI is sodium carbonate, Na2CO3. A measured mass of solid Na2CO3, mNa2CO3' in grams, is dissolved in water and then titrated with HCI solution using methyl 2 NaCl + CO2 + H2O. orange indicator. The reaction is: Na2CO3 + 2 HCI- Complete the following formulas using the context described above: MHCI × VHCI in mL at the methyl orange endpoint = mNa2CO3 × ( )= mol of Na2CO3 mol of Na2CO3 X (— ( - - )= mol of HCl
Hh.132.
7. (8 pts) Calculate the solubility product, Ksp, for SrF2, given that its solubility is 0.0080 g per 225.0 mL of solution. SrF (s)  Sr2 (aq)  2F  (aq) 2
Given are the following reactions: Reaction #1 N2H4(l)+O2(g)⟶N2(g)+2H2O(g) ΔH⊖reaction= -534.2 kJkJ Reaction #2 H2(g)+1/2O2(g)⟶H2O(g) ΔH⊖reaction = -241.8 k a. what is the reversed reactions equation? b. what is delta h of the reversed reaction?
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(-57)2 (3.145)3(1:715) 19. At a high temperature, equal concentrations of 0.160 mol/L of H2(g) and I2(g) are initially present in a flask. The H2 and l2 react according to the balanced equation below. H2(g) + I2(g) → 2 HI(g) When equilibrium is reached, the concentration of H2(g) has decreased to 0.036 mol/L. What is the equilibrium constant, Ke, for the reaction? а. 3.4 b. 4.0 С. 12 d. 22 e.) 48
Help with the CHEM Lab report please! It is about Volumetric Analysis There is also a Burn trail please make sure for that!

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