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How will the solubility of calcite change as a function of temperature? Justify your answer in terms of thermodynamics. This is what I have so far.... Solubility of calcite (CaCO3) will increase with a decrease in temperature and decrease with an increase in temperature. This is because the solubility of calcite is dependent on the solubility of CO2.
A 1 L flask is filled with 1.45 g of argon at 25 C}. A sample of ethane vapor is added to the same flask until the total pressure is 1.25 atm.what is the partial pressure of argon in the flask?
A 0.30 M solution of sucrose (C12H22O11) at 37oC has approximately the same osmotic pressure as blood. What is the osmotic pressure of blood?
Based on Liquid Chromatography, how can I changed if the capacity value and selectivity value and resolution value is not in the proper range?
Calculate the net charge of Aspartic Acid. Its given that Aspartic acid has a pK1 COOH at 1.99 and also a pK2 NH3 group at 9.90
Calculate the molarity of each of the following solutions(a) 29.0 g of ethanol (C2H5OH) in 545 mL of solution.
what are the hydrolysis by-products? What limits the reaction? What determines whether the hydrolysis reaction proceeds from cellulose to sugar (e.g. glucose) or continues on to convert the sugars to alcohol?
An aqueous solution is 22.0% by mass ethanol, CH3CH2OH, and has a density of 0.966 g/mL. what is molality of ethanol
Calculate the concentrations of each of the ions in 0.12 M (NH4)2HPO4. a) [NH4+], M b) [HPO42-], M
what is the ratio of the rate of reaction A to reaction B ? B) if the initial concentrations of the reactants are both 1.80 M, what is the ratio of the rate of reaction A to reaction B ?
Determine the pH and the percentage of fully protonated weak acid/base for each of the solutions listed below:
Lethality of Carbon Monoxide, Sulfur Dioxide and TNT Air monitoring provides the following contaminant concentrations at the approximate center of a fire scene in which acres of automobile tires are burning:
Calculate what the limiting reactant is in the reaction between copper (II) oxide and hydrochloric acid
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