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You have a solution of a buffer with 10 mMoles of the buffer. Initially the solution has a pH of 6.8. You add 100 mM kOH and the pH rises to 7.1. The pKa of the buffer is 6.3.
How many mls of KOH did you add?
In an earlier problem we described the reaction of ammonia with oxygen to form nitrogen monoxide, NO.4NH3 + 5O2 ? 4NO + 6H2O
an aqueous cacl2 solution has a vapor pressure of 82.1 mmhg at 50 c . the vapor pressure of pure water at this
Calcein indicator is added to the solution. The sample then requires 10.00 mL of 0.0120 M EDTA for titration. Calculate for this sample (a) the molarity of the calcium present, (b), the molarity of the magnesium present, and (c) the total hardness..
Calculate the pH of 1.00 L of the buffer 1.00 M CH3COONa/1.00 M CH3COOH before and after the addition of (a) 0.080 mol NaOH, (b) 0.12 mol HCl. (Assume that there is no change in volume.)
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Find the new volume of the gas sample - What is the new volume of the gas sample
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What mass of solid citric acid (g) and how many milliliters of 0.500 M NaOH are needed to produce 100.0 mL of a buffer with a pH of 6.50 and a weak base concentration of 0.0250 M
Exactly 100 mL of 0.10 M nitrous acid (HNO2) are titrated with a 0.10 M NaOH solution. Calculate the pH for the following. (a) the point at which 80 mL of the base has been added
Understanding the basics of thermal chemistry and The Second Law of Thermodynamics indicates that a system
Use the ideal gas law to calculate the concentrations of nitrogen and oxygen present in air at a pressure of 1.0 and a temperature of 298 .
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