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Write equations and show how the following molecules can be prepared from any organic and inorganic reagents.
1. cyclohexane-S-CH2-CH3
2. H3C-C(CH3)2-O-CH2-CH3
3. C4H8O (Cyclo)
4. CH3CH2NH2
Calculate the pH of a buffer composed of .50 M formic acid (HCO2H) and .70 M sodium formate (HCO2-Na+) before and after the addition of 10.0 ml of 1.0 M HCL
how many grams of water are consumed if 4.0 g of hydrogen gas and 32.0 g of oxygen are produced
A 0.479 g sample of nitrogen, oxygen or neon gas occupies a volume of 265 mL at 157 kPa and 20?C. What is the molar mass and identity of the gas
Given the pK for acetic acid is 4.76. Suppose that we dissolve a mole of this weak acid in 10L of water. Find the pH of the resulting solution.
A student wanted to determine the molar concentration of acetic acid in a commercial vinegar sample. He used a volumetric pipet to deliver 3.00 mL of vinegar to an Erlenmeyer flask, added about 30 mL of water and 3 drops of phenolphthalein indicat..
Calculate the pressure and the temperature of the compressed gas. In a diesel engine the compression ratios are typically much higher; redo the same calculation for the compression ratio of 20:1.
the total volume of hydrogen needed to fill the Hindenberg was 2.0x10^8 L at 1.00 atm and 25 C. How many kilojoules of energy were evolved when it burned?
Does the effective buffer range of a buffer solution depend on the concentrations of the conjugate acid and base pairs in the buffer solution
Is the dissociation of NaCl reversible. When you dissolve it in water does it dissociate and associate back together
Formalin is an aqueous solution of formaldehyde, HCHO, used as a preservative. How many grams of formaldehyde must be used to prepare 2.5 L of 12.3 M solution
Oxygen gas is commonly sold in 45.5 L steel containers at a pressure of 131 atm . What volume (in liters) would the gas occupy at a pressure of 1.06 atm if its temperature remained unchanged
When 75.0 mL of a 0.100 M lead (II) nitrate solution is mixed with 100.0 ml of a 0.190 M potassium Iodide solution, a yellow-orange precipitate of lead (II) iodide is formed.
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