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A solution of I2 was standardized with ascorbic acid. Using a 0.100 g sample of pure ascorbic acid, 25.32 ml of I2 were required to reach the starch end point.a) what is the molarity of the iodine solutionb) what is the titer of the iodine solution
Determine the mass of phosphorus (P) is required to make 39 grams of this product?
Find the concentration and pH solution - What is the pH of a solution of 0.65 M acid and 0.51 M of its conjugate base if the pKa = 5.30?
A certain solid metallic element has a density 7.87 g/cm3 and a molar mass of 55.85 g/mol. It crystallizes with a cubic unit cell, with an edge length of 286.7 pm. calculate the number of atoms per unit cell.
Sucrose, C12H22O11, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte.
A 270- flask contains pure helium at a pressure of 755 . A second flask with a volume of 485 contains pure argon at a pressure of 727 torr.
Methane has a Henry's Law constant (k)of 9.88 × 10-2 mol/(L·atm) when dissolved in benzene at 25°C. How many grams of CH4 will dissolve in 3.00 L of benzene if the partial pressure of CH4 is 1.48 atm?
A gas measures 180.0 mL at 87.0°C and 800.0 mm. Find its volume at standard temperature and 800.0 mm of pressure.
The heat of vaporization of water is 40.66 kJ/mol. Assuming sweat is 100% water, how much heat is removed from your body through the evaporation of 3.13 g of sweat?
Compute the concentrations of all species in a 0.900 M sodium sulfite solution. If it is given that the ionization constants for H2SO3 are Ka1=1.4x10^-2 and Ka2=6.3x10^-8.
A 62g piece of ice at 0 degree celsius is added to a sample of water at 9 degree celsius. All of the ice melts and the temperature of the water decreases to 0degree celsius. How many grams of water were in the sample ?
A buffer is made by dissolving H3PO4 and NaH2PO4 in water. Write and equation that shows how this buffer neutralizes added bases.
Single double triple bonding, Explain the characteristics of a single, double, and triple bonds including why they form and how the electrons
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