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Calculate the ksp of a solution containing 0.150 M PbI2.
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- 9. We prepared a solution containing 1.0 mol.L' HF and 1.0 mol.L·' C,H3OH. The K, of hydrofluoric acid and phenol are 7.2 x 104 and 1.6 x 10-10 respectively. What is the pH of this solution? (Hint: find which acid is strongest and make the appropriate assumptions) b. What is the concentration of C,H;O¯ at equilibrium? а.The solubility (denoted as s) of CaSO4 in pure water at 40o C is 1.09 grams per liter. What is the value of the solubility product of CaSO4?A 1.00 liter solution contains 0.52 moles hypochlorous acid and 0.40 moles potassium hypochlorite. If 0.20 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) A. The number of moles of HC1O will decrease. ⒸB. The number of moles of C10¯ will remain the same. C. The equilibrium concentration of H3O+ will decrease. ⒸD. The pH will remain the same. [HCIO] [C10¯] ⒸE. The ratio of will increase.
- A 1.00 liter solution contains 0.35 M hypochlorous acid and 0.26 M potassium hypochlorite. If 30.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water.) A. The concentration of HClO will remain the same. B. The concentration of ClO- will increase. C. The equilibrium concentration of H3O+ will decrease. D. The pH will remain the same. E. The ratio of [HClO] / [ClO-] will remain the same.A 1.00 liter solution contains 0.33 moles nitrous acid and 0.25 moles potassium nitrite . If 0.13 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) JA. The number of moles of HNO2 will remain the same. B. The number of moles of NO2 will decrease. |C. The equilibrium concentration of H30* will decrease. D. The pH will increase. E. The ratio of [HNO2] / [NO2] will remain the same.3. The solubility of CsF2(s) in water is 2.1 x 104 M. Calculate its Kap.
- A student titrates 20.0 mL of 1.0 M NaOH with 2.0 M formic acid, HCOOH (K, = 1.8 x 104). Hypochlorous acid is an unstable compound and one of the decomposition products is chlorine gas, Cl2. The composition of the acid lowers its concentration over time. What effect will the decomposition of one-fourth of the acid have on the agreement between the endpoint of the titration and the equivalence point during a titration with standard sodium hydroxide? It is impossible to determine The endpoint would be before the ideal equivalence point The endpoint would be after the ideal equivalence point The endpoint will rema eerthe ideal egvaleacepolntA 1.00 liter solution contains 0.34 M nitrous acid and 0.44 M potassium nitrite. If 0.110 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) VA. The number of moles of HNO2 will decrease. vB. The number of moles of NO2 will remain the same. C. The equilibrium concentration of H30+ will remain the same. D. The pH will decrease. E. The ratio of [HNO2] / [NO2] will decrease.A 1.00 liter solution contains 0.60 moles nitrous acid and 0.46 moles potassium nitrite .If 0.23 moles of perchloric acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of HNO2 will increase. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase.
- 0.0500 M HF (Ka= 7.20 x 10–4) determine the equilibrium molar concentration of H3O+ and equilibrium molar concentration of HF (in 3 sig. figures).What weight of potassium hydrogen phthalate will require 30. mL of a 0.30M NaOH solution to reach the equivalence point? KHP MM 204.22 g/mol .CO;K' .CO;K' NaOH + H2O + *CO,H COƠ,Na'In an experiment, 1.000 mol H and 1.000 mol I2 are mixed in a 1.00-L container, and the reaction forms HI. If K. = 54.3 for this reaction, what is the enuilibrum concentration of HI? 12(g) H2(g) 2HI(g) +. O a. 1.572 O b.0.226 O c. 0.399 O d.0.786 O e.0.899 Question 3 Moving to the next question prevents changes to this answer. Σ