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An aqueous potassium nitrate solution has a freezing point of -2.0 °C. How many moles of potassium nitrate are contained in 0.5 kg of water in this solution? The freezing point depression constant for water is -1.86 °C/m.
Write the ionic equation for the reactions. Write the net ionic equations for the reactions, A.) LA2(CO3)3 (s)+HCL (aq)= LaCl3 (aq) + CO2 (g) + H20
Historically, the solid residue that is left after the methylene chloride solution is evaporated has a lower melting point that its literature value, due to impurities. Explain what impurities are present and why.
How much heat is required to take a 15.0 g sample of ice with an initial temperature of 0.00oC and raise it to a final temperature of 75.0 oC.
Find the pH and fraction of dissociation of a 0.100 M solution of the weak acid HA with Ka= 1.00 x 10-5.
We assume the first step in this decay series is, by far, the slowest and that all the 206Pb found in the sample is derived from this decay process. How old (in billions of years, where 1 billion = 109) is the rock
If the concentration of bromide ion in a saturated solution in equlibrium with PbBr2 solid is determined to be .0125M what is the solubility of PbBr2
If you wanted to prepare a 1.45 L buffer with a total phosphate concentration of 0.0500 M, how many grams of NaH2PO4 and Na2HPO4 would you mix together? How many grams of conjugate acid do you need? How many grams of conjugate base do you need?
How much heat is gained (in Joules) by the water where a chemical reaction takes place in 100 mL aqueous solution and has a temperature increase of 14 C?
Identify the unknown gas - Find the molecular formula of the compound
an optically pure compound was diluted to 200.0 mL with water and placed in a polarimeter tube 10.0 cm long. The measured rotation was -2.53° at 25 °C. Calculate the specific rotation of the compound.
A zero-order reaction has a constant rate of 3.20×10-4 . If after 60.0 seconds the concentration has dropped to 6.50×10-2 , what was the initial concentration?
An 11.0 gram sample of CO2 exerts a pressure of 50.0kPa. What mass of CH4 must be added to the CO2 in order to increase the pressure of 75.0 kPa? Assume no CO2 escapes.
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