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If 2.00mL of 0.0850 M NaOH is added to 75.0mL of the buffer solution, Explain what will be the pH of the final solution?Problem 1: Explain what is the pH of a buffer solution that is 0.245 MCH3NH2 methylamine and 0.186 MCH3NH3Cl methyl ammonium chloride?
A solution containing both Mn2+ and Cd 2+ is saturated with H2S gas, after which the concentration of H is found to be .30 M. will the sulfides of these ions form a precipitate under these conditions
A solution of 2.00 g of Para-dichlorobenzene a clothes moth repellant in 50.0g of cyclohexane freezes at 1.05 deg C. Explain what is the molar mass of this substance
Solve for the new pressure in each of the following, with n and V constant: 1)A gas with a pressure of 1.25 atm at 90 Celsiusis cooled to -17 Celsius. 2)A sample of N2 with a pressure of 790 mm Hg at -75 Celsius is heated to 34 Celsius
A solution is made by dissolving 0.150 moles of benzoic acid (ka=6.5*10^-5) and 0.300 moles of sodium benzoate in enough water to give exactly 1.00 L of solution what is the solution pH
A sample of propane,C3H8, contains 11.7 moles of carbon atoms. How many total moles of atoms does the sample contain?
Although coals is a complex mixture of substances, its elemntal composition can be approximated by the formula C135H96O9NS. Using this formula calculate the mass of carbon in 1.00 x 10^9 kg of coal
Sodium-24 has a half-life of 15.0 hours and is used to study blood circulation. If a patient is injected with 20.0 grams of Na-24 (usually done in the form of 24NaCl), how much is still present in the patient after 4.0 days?
What is the difference between July and January temperatures in the Celcius scale? What is the difference between July and January temperatures in the Kelvin scale?
what is the percentage ionization of the benzoic acid in the resulting solution. Ka(benz acid)=6.5 * 10^-5
What is the freezing point of a solution prepared by dissolving 11.3 g of Ca(NO3)2 in 115 g of water?
Determine the moles of H2O lost. E. Write the empirical formula for hydrated alum, based on your experiment.
A quantity of N2 occupies 62.2 L at a particular temperature and pressure. Its density is 0.900 g/L. How many moles of N2 are in the container?
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