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Chapter 20: Problem 36
Write a balanced equation describing the reaction of aluminum metal with concentrated aqueous sodium hydroxide.
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The electrolysis of aqueous sodium chloride (brine) is an important industrial process for the production of chlorine and sodium hydroxide. In fact, this process is the second largest consumer of electricity in the United States, after the production of aluminum. Write a balanced equation for the electrolysis of aqueous sodium chloride (hydrogen gas is also produced).
Fluorine reacts with sulfur to form several different covalent compounds. Three of these compounds are \(\mathrm{SF}_{2}, \mathrm{SF}_{4},\) and \(\mathrm{SF}_{6} .\) Draw the Lewis structures for these compounds, and predict the molecular structures (including bond angles). Would you expect \(\mathrm{OF}_{4}\) to be a stable compound?
Use the symbols of the elements described in the following clues to fill in the blanks that spell out the name of a famous American scientist. Although this scientist was better known as a physicist than as a chemist, the Philadelphia institute that bears his name does include a biochemistry research facility. (1) The oxide of this alkaline earth metal is amphoteric. (2) The element that makes up approximately 3.0% by mass of the human body. (3) The element having a 7\(s^{1}\) valence electron configuration. (4) This element is the alkali metal with the least negative standard reduction potential. Write its symbol in reverse order. (5) The alkali metal whose ion is more concentrated in intracellular fluids as compared with blood plasma. (6) This is the only alkali metal that reacts directly with nitrogen to make a binary compound with formula \(\mathrm{M}_{3} \mathrm{N}\). (7) This element is the first in Group 3A for which the 11 oxidation state is exhibited in stable compounds. Use only the second letter of its symbol.
Calculate the solubility of \(\mathrm{Mg}(\mathrm{OH})_{2}\left(K_{\mathrm{sp}}=8.9 \times 10^{-12}\right)\) in an aqueous solution buffered at \(\mathrm{pH}=9.42 .\)
EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt $\mathrm{Na}_{2} \mathrm{H}_{2} \mathrm{EDTA}$ , are also used to treat heavy metal poisoning. The equilibrium constant for the following reaction is \(6.7 \times 10^{21} :\) Calculate \(\left[\mathrm{Pb}^{2+}\right]\) at equilibrium in a solution originally 0.0050 \(\mathrm{M}\) in \(\mathrm{Pb}^{2+}, 0.075 M\) in \(\mathrm{H}_{2} \mathrm{EDTA}^{2-},\) and buffered at \(\mathrm{pH}=7.00 .\)
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