Q: How to balance this chemical equation? KO2(s) +H2O(l) ----> KOH(aq) + O2(g) + H2O2
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Q: Fe) + H20)→ Fez04(8) + H 29) | b. How many moles of Fez04 can be produced from 6.0 mol of Fe?
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- Both AgCl and Agl dissolve in NH3.. (a) What mass of AgI dissolves in 1.0 L of 1.0 M NH3?. (b) VNhat mass of AgCl dissolves in 1.0 L of 1.0 M NH3?For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
- What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.What's molar solubility of Ca(OH)2 in water using the systematic method?Q: The solubility product of Zn(OH)2 at 25oC is 3.0 x 10-6 M3. Calculate the solubility of Zn(OH)2 in water in gdm-3. [Ar: Zn = 65.5; O = 16; H = 1] The Mr for Zn(OH)2 is 99.5. When I multiply it with Ksp, I didn't get the same answer as the given answer which is 0.904 gdm-3.
- 100 ml 0.10M AgNo3 is added 100 ml of 0.12 M Nacl (ksp agcl = 1x10^-10) 1. CALCULATE THE NUMBER OF MILLIGRAMS of Ag+ not precipitate (m. W of ag = 107.8 g/mol) 2. If precipitate of agcl is washed with 200 ml of water at 25 c what is yhe maximum number of milligrams of agcl that could be lost by solubility in the wadh water? ( m. W agcl = 143,32 g /mol)Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 12.15 mL of 0.250 M NaOH to reach the phenolphthalein endpoint. How many grams of acetic acid are present in the sample?1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…
- The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?Calculate the solubility (in M) of cobalt(II) hydroxide, Co(OH)2(s) in H2O. Ksp = 1.70×10-16 at a specific temperature.