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Calculate the mass of sodium required to produce 80 grams of sodium hydroxide by direct reaction with water: 2Na(s) + 2H2O(l) = 2NaOH(aq) +H2(g) (s) = solid, (l) = liquid, (aq) = water solution aqueous mixture and (g) = gasa. 33.2 grams Na
b. 46 grams Na
c. 58.4 grams Na
d. 78.94 grams Na
e. 84.8 grams Na
A certain lead-sulfur compound contains 86.59% Pb by mass and the remainder is sulfur. What is the empirical formula of the compound
write the net ionic equation for a solution of calcium chloride and a solution of mercury(1) nitrate
Indicate the hybridization for each carbon and nitrogen atom in this molecule, then draw an orbital overlap picture for the molecule.
Calcium reacts with iodine to form an ionic compound. If a sample of the compound contains 8.5 x 1019 iodide ions, how many calcium ions does it contain?
An excited hydrogen atom with an electron in the n=5 state emits light having frequency of (6.9 x 10^14)(s^-1). what is the principle quantum level for the final state in this electronic transition
The concentration of Na^+ in a 0.73 M Na2CO3 solution is: (Assume complete dissaciation) A. 0.43 M B. 0.88 M C. 1.02 M D. 1.28 M E. 1.46 M
A buffer is prepared by mixing 500 ml of 0.4 M Na2HPO4 and 500 ml of 0.2 M NaH2PO4 (pK1 = 2.10; pK2 = 6.70; pK3 = 12.30). Calculate the pH of this buffer.
For the chemical equations shown below, label each reactant as either acid or base, and each product as either conjugate acid or conjugate base according to the Brønsted-Lowry definition.
A stock solution of NaCl is made taking 150.2g in enough water to make 200.0ml. A 10.00 ml sample of this stock solution is diluted to 250.0 ml.
What concentration of CH3NH3Br is necessary to prepare a pH = 10.00 buffer solution assuming the base concentration is 0.67 M (Kb for CH3NH2 = 4.4 x 10-4). For this problem, include the correct units of M.
A gas system has initial volume and temperature of 8160mL and 467.0K. If the temperature changes to -151C, what will the resultant volume be in mL
500 mL of 0.1 M NaOH is added to 585 mL of 0.25 M weak acid (Ka = 2.21 x 10^-5). What is the pH of the resulting buffer?
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