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Calculate the molarity of a Ca(OH)2 solution if it takes 25.0 mL to titrate 0.650 g of KHP in a standardization titration. (KHP has one H+ and a formula weight of 204.2 g/mol.)
How many independent linear combinations are possible for four 1s orbitals? (b) Draw pictures of the linear combinations of H1s orbitals for a hypothetical linear H4 molecule
a step by step answers for those Question please. Please be brief. What is the PH of a buffer prepared by combining 25mL of 0.1M nitrous acid with 25mL of 0.1M sodium nitrite?
These 3 solutions including 2.362 g of Rb2S, 1.635 g of NaClO 4 , and 0.796 g of CuCl 2 , respectively are combined together? now calculate what would be the mass of this precipitae?
What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?
When 228.4 mg of pure X was burned 627.4 mg of CO2 and 171.2 mg of H2O were obtained. Determine the simplest formula of the compound X.
Write the expression for the equilibrium constant, Kb, for methylamine also compute the molar concentration of OH- in the 50.0 mL sample of the CH 3 NH 2 solution.
At what pH will a solution 0.15 M Cu2+ begin to precipitate as Cu(OH)2? The Ksp for Cu(OH)2 is 1.6 × 10-19.
Meaning, use and calculation of empirical formulas, In this introduction are given the explanation of how to find out an empirical formula if one has found out the chemical elements of an unknown substance and measured their ratio of masses
To determine the freezing points of distilled water, 1m glucose, 1m NaCl, 1m CaCl2. Use the freezing point of the pure water as a baseline to determine deltaTf for each of the solutions
Why is it necessary to first "process" the broccoli before preparing the test sample? What factors are affected that will adversely influence
When an ionic solid is added into a solvent, you can see that the ionic solid dissociates into its respective cations and anions. The solvent molecules immediately cluster around the ions.
Consider a glass of 215 mL of water at 28°C. Calculate the mass of ice at -15°C that must be added to cool the water to 10°C after thermal equilibrium is achieved.
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