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In the lab experiment you carefully collect all of the gas formed and find that there is 425.6mL of gas. What is your percent yield?
Write a chemical equation for the following reactions: zinc sulphate + barium nitrate.
Commercial steric acid (C17H35COOH) contains palmatic acid (C15H31COOH) as an impurity. If a 1.115 gram sample of commerical steric acid is dissolved.
Using Ostwald process, what mass of nitric acid could be produced from 75.0 g of N2 and 50.0 g of H2?
One gram of NaCl and one gram of sand are added to 100mL of water. What is the solvent?
How many moles of chloride ions are in 250.0mL of a 0.450M calcium chloride solution?
If 500 mg/L lactic acid is added to pure water and you add NaOH until the pH = 3.1, what are the final amounts of each species in the acid equilibrium?
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 and pH is 4.20.
What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1 liter of solution buffered at Ph of 3.55?
What are the equations for these metals when mixed with 6 M HCl. Ca, Cu, Mg, Fe, Sn, and Zn. (I tried Ca + HCl and got 3 Ca + 6HCl --> 3CaCl2 + 3H2)
Into a 5.0 liter flask was placed 35.7 g of PCI5 . The flask and contents were heated to 250 0 C, and then held at temperature.
The only possible ions in an aqueous solution are ion, barium, carbonate, chloride and nitrate.
When iron is oxidized in the presence of nitric acid, three products are formed: iron(III) oxide, nitrogen dioxide and water.
A weak acid has a PKa of 7.713. Calculate the pH of a solution in which the ratio of the concentrations of undissociated acid to acid anion ([HA]/[A-]).
Calculate the pH of a solution in which the ratio of the concentrations of acid anion to undissociated anion ([A-]/[HA]) equals 7.555.
The gaseous hydrocarbon acetylene, C2H2, is used in welders torches because of the large amount of heat released when acetylene.
Is it possible to calculate concentration of a solution, OH- concentration, and H+ concentration from just a pH given (no specific base or acid)?
A diprotic acid, H2A, has the following ionization constants: Ka1 = 1.1E-3 and Ka2 = 2.5E-6. In order to make up a buffer solution of pH 5.8.
Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer.
A reacts spontaneously with 1mol/L BNO3, 1mol/L D(NO3)2 and dilute sulfuric acid.A does not react with 1mol/L C(NO3)2.
A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL
If equal molar amounts of Na2HPO4 and NaJpo4 are mixed in water, calcuate the resulting pH. The pKas of phosphoric acid are 2.1, 7.2, 12.4.
Which is the correct order of increasing (from least to most reactive) activity for these metals?
With a Ka = 5.8 x 10^-10 it is a weak acid that behaves as a monoprotic acid. Assume you titrate 20.0 mL of 0.11 M boric acid with 0.100 M NaOH. (Show work)
What is the name of the salt formed by the complete neutralization of sulfuric acid with lithium hydroxide?