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The solution was boiled to remove CO2, following which the excess HClO4 was back-titrated with 10.12ml of dilute NaOH. In a separate experiment, it was established that 27.43 ml of HClO4 neutralized
A sodium hydroxide solution is prepared by dissolving 4.0 g NaOH in 1.00 L of solution. What is the molar concentration of OH- in this solution? What are the pOH and the pH of the solution?
A solution of HClO4 was standardized by dissolving .4125g of primary-standard-grade HgO in a solution of KBr. The liberated OH consumed 46.51mL of the acid. Calculate the molarity of the HClO4.
Consider the following reaction at constant P. Use the information here to determine the value of ?Ssurr at 355 K. Predict whether or not this reaction will be spontaneous at this temperature.
What is the molar solubility of magnesium carbonate ( MgCO3 ) in water? The solubility-product constant for MgCO3 is 3.5 × 10-8 at 25°C.
A second 50ml aliquot was brought to a pH of 10 with an HCN/NaCN buffer, which also served to mask Cd2+; 11.56 ml of EDTA solution were needed to titrate the Pb2+. Calculate the percentage of Pb and
The Tl in a 9.76 g sample of rodenticide was oxidized to the trivalent state and treated with an unmeasured excess of Mg/EDTA solution. The reaction is Tl3+ +MgY2-> TlY- + Mg2+
The de Broglie wavelentgh of an electron is 8.7 x 10^-11m. The mass of this electron is 9.1 x 10^31 kg. What is the velociy in m/s of this electron (h = 6.63 x 10^-34 J-s)
The excess reagent required 4.30mL back-titration with .00812M Cu2+. Calculate the average weight of Cr on each square centimeter of surface.
Although the use of absorbances at 450 nm provided you with maximum sensitivity, the absorbaces at, say, 400 nm or 500 nm are not zero and could have been used throughout this experiment. would the
canned tuna was analyzed by the Kjeldahl method; 22.66ml of .1224M HCl were required to titrate the liberated ammonia. Calculate the percentage of nitrogen in the sample.
which caused the CO2 in the sample to precipitate as BaCO3. The excess base was back-titrated to a phenolphthalein end point with 23.6ml of .0108 M HCl. What is the concentration of CO2 in the air i
1401g sample of a purified carbonate was dissolved in 50ml of a .1140 M HCl and boiled to eliminate CO2. Back titration of the excess HCl required 24.21ml of .09802M NaOH. Identify the carbonate.
What are the coefficients of the reactants and products in the balanced equation above? Remember to include H2O(l) and H+(aqu) in the appropriate blanks.
A 50ml sample of a white dinner wine required 21.48 ml of .03776 M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in terms of grams of tartaric acid (150.09g/mol) per 1
Identify the species that is oxidized and the species that is reduced in each reaction.Write out two half reaction to show how many electrons are gained or lost by each species.
A gas expands and does P-V work on the surroundings equal to 313 J. At the same time, it absorbs 135 J of heat from the surroundings. Calculate the change in energy of the gas.
which one of the following represents the best method for the preparation of 3-chloro-3 ethylpentane?
The formaldehyde content of a pesticide preparation was determined by weighing .3124g of liquid sample into a flask containing 50ml of .0996M NaOH and 50mL of 3%H2O2. On heating, the following react
A sample of gas occupies a volume of 692 mL at 1.24 atm and 85 oC. Calculate the pressure of the gas if its volume is changed to 484 mL while its temperature is held constant.
Five constituionally isomeric monochlorides of molecular formula c6h13cl are formed (along with a mixture of dichlorides, trichlorides, etc.) What is the most reasonable structure for the starting a
Calculate the number of moles of an ideal gas if it has a pressure of 1.02 atm, a volume of 2.76 L, and a temperature of 222 oC. Use R = 0.0821 L-atm/mol-K for the value of the gas constant.
Titration of a .7439g sample of impure Na2B4O7 required 31.64mL of .1081M HCl. Express the results of this analysis in terms in percent
A mixture of gases contains 5.31 g of He, 2.91 g of SO2, and 5.62 g of Ne. If the total pressure of the mixture is 3.81 atm, what is the partial pressure of each component
A mixture of gases contains 4.32 g of Ar, 7.88 g of BF3, and 4.86 g of N2. What is the partial pressure in atm of each component of this mixture if it is held in a 61.3-L vessel at 10.9 oC? Use R =