Chapter 4: Problem 2
The average adult has about \(16 \mathrm{~g}\) of sodium ions in her blood. Assuming a total blood volume of \(5.0 \mathrm{~L}\), what is the molarity of \(\mathrm{Na}^{+}\) ions in blood?
Chapter 4: Problem 2
The average adult has about \(16 \mathrm{~g}\) of sodium ions in her blood. Assuming a total blood volume of \(5.0 \mathrm{~L}\), what is the molarity of \(\mathrm{Na}^{+}\) ions in blood?
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Get started for freeSolid iron(III) hydroxide is added to \(625 \mathrm{~mL}\) of \(0.280 \mathrm{M} \mathrm{HCl}\). The resulting solution is acidic and titrated with \(238.2 \mathrm{~mL}\) of \(0.113 \mathrm{M} \mathrm{NaOH}\). What mass of iron(III) hydroxide was added to the HCl?
I A student is given \(0.930 \mathrm{~g}\) of an unknown acid, which can be either oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), or citric acid, \(\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\). To determine which acid she has, she titrates the unknown acid with \(0.615 \mathrm{M} \mathrm{NaOH}\). The equivalence point is reached when \(33.6 \mathrm{~mL}\) are added. What is the unknown acid?
Iodine reacts with thiosulfate ion, \(\mathrm{S}_{2} \mathrm{O}_{3}{ }^{2-}\), to give iodide ion and the tetrathionate ion, \(\mathrm{S}_{4} \mathrm{O}_{6}{ }^{2-}\). (a) Write a balanced net ionic equation for the reaction. (b) If \(25.0 \mathrm{~g}\) of iodine is dissolved in enough water to make \(1.50 \mathrm{~L}\) of solution, what volume of \(0.244 M\) sodium thiosulfate will be needed for complete reaction?
Write a balanced net ionic equation for each of the following acidbase reactions in water. (a) nitrous acid and barium hydroxide (b) potassium hydroxide and hydrofluoric acid (c) aniline \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\right)\) and perchloric acid
The percentage of sodium hydrogen carbonate, \(\mathrm{NaHCO}_{3}\), in a powder for stomach upsets is found by titrating with \(0.275 M\) hydrochloric acid. If \(15.5 \mathrm{~mL}\) of hydrochloric acid is required to react with \(0.500 \mathrm{~g}\) of the sample, what is the percentage of sodium hydrogen carbonate in the sample? The balanced equation for the reaction that takes place is $$ \mathrm{NaHCO}_{3}(s)+\mathrm{H}^{+}(a q) \longrightarrow \mathrm{Na}^{+}(a q)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O} $$
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