12.59 Place the following solutions in order of increasing [H3O+]. Please explain your reasoning.
0.10 M HF, 0.10 M NH3, 0.10 M HNO3
0.10 M HCN, 0.20 M HCN, 0.20 M HClO4
0.10 M NH3, 0.10 M NaOH, 0.10 M Ca(OH)2
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12.59 Place the following solutions in order of increasing [H3O+]. Please explain your reasoning. 0.10 M...
Rank the following 0.10 M solutions in order of increasing pH. (Use the appropriate <, =, or > symbol to separate substances in the list.) (a) RbF, RbBr, HBr, HF (b) LiI, NH4I, HI, NH3 (c) RbOH, RbOBr, HONH3ClO4, HOBr, HClO4, HONH2, RbClO4
Rank the following 0.10 M solutions in order of increasing pH. (Use the appropriate <, =, or > symbol to separate substances in the list.) a) RbClO4, HONH2, HClO4, RbOH, HONH3ClO4, RbOBr, HOBr
Rank the following 0.10 M solutions in order of increasing pH. (c) LiOH, LiClO4, HONH3ClO4, LiOBr, HClO4, HOBr, HONH2
Rank the following 0.100 M solutions in order of increasing H3O+ concentration: HOCl, Ka = 4.0 x 10-8; HCN, Ka = 6.2 x 10-10; NH4+, Ka = 5.6 x 10-10
Arrange the following 0.1 M solutions in order of increasing pH and state why you placed each solution in that position: NaCH3COO, HCl, HCN, NaOH, NH3, NaCN, KNO3, H2SO4, NH4Cl, H2SO3, NaHCO3, Na3PO4 and CH3COOH. please list each solution in order and next to it be specific next to each in terms of why each solution was placed in its respective position - please include ka and kb values in your explanation while ranking the solutions and add in any...
Arrange the group of compounds and ions/ in order of increasing pH? 1) NH4Cl, H2SO4, NaOH,Na2CO3 2)H2Se,HI,H2S,NH3 3) HCLO, HClO3,CLO^-, HBrO 4) K2SO3, Ca(OH)2, HCL,HF 5) NH3, H3O+, OH^-, HF
1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O. 2. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side...
Place the following species in order of increasing Brønsted acidity and briefly explain your reasoning: H3AsO3, H2AsO2-, H3AsO4, H2SO4, H2SeO4.
We have (a) 50.0 mL of 0.10 M NH3 solution, (b) 50.0 mL of 0.12 M HNO3 solution, (c) 50.0 mL of 0.12 M NaOH solution, and (d) 50.0 mL of 0.06 M HClO4 solution. Can you make a buffer by combining two of these solutions? If so, which ones? What would be the pH of the buffer solution? Please explain
QUESTION 3 Place the following solutions in order of increasing osmotic pressure. (Hint: the solutes are l. molecule, II. a soluble ionic and III. a weak acid). I.0.15 M C2H6O2 II. 0.15 M NaCI III. 0.15 M HFQUESTION 4 Place the following aqueous solutions of nonvolatile, nonionic compounds in order of decreasing osmotic pressure. I. 0.011 M sucrose II. 0.0095 M glucose III. 0.0060 M glycerin