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Calculate the pH and the pOH of an aqueous solution that is 0.040 M in HCl(aq) and 0.065 M in HBr(aq) at 25°C.
The answer isnt pH1.28 and pOH 12.72
Hydrogen peroxide undergoes a first-order decomposition to water and O2 in aqueous solution. The rate constant at 25 °C is 7.40 * 10-4 s-1. Calculate the volume of O2 obtained from the decomposition of 1.00 mol H2O2 at 25 °C and 740 mmHg after 20...
Consider the reaction 4KO2(s) + 2CO2(g)->2K2CO3(s) + 3O2(g) . How much KO2 is needed to react with 75.0 L of carbon dioxide at STP?
An aqueous solution is made by dissolving 25.8 grams of magnesium nitrate in 395 grams of water. What is the molality of magnesium nitrate.
A 75.0-mL volume of 0.200 NH3 is titrated with 0.500 M HNO3 . Calculate the pH after the addition of 19.0 mL of HNO3
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The average mass of a carbon atom is 12.011. Assuming you were able to pick up only one carbon atom, the chances that you would choose a carbon atom with a mass of 12.011 is:
The first steps in the radioactive decay of 257 Uuh involves the rapid and successive emission of 2 alpha particles. [Note: Uuh is the symbol for ununhexium, which is element number 116.]
A gas has an initial volume of 2.75 L at temperature of 285 K. If the temperature changes to 380 K, what is the new volume of the gas if the pressure is unchanged?
calculate the external pressure that must be applied to seawater, 1.14 M total ion concentration at 10 degrees celcius if the maximum concentration allowed in the product water is 166 mg/L
The minimum energy required to cause the photo electric effect in potassium metal is 3.69*10^-19 J. will photoelectrons be produced when light shines on the surface of potassium?if 400 nm radiation is shone on potassium,what is the velocity of the..
Nickel is a transition element and has a variable valence.Using a nickel salt, 2 F (faradays) plate out 39.2 g ofnickel. What ions are in the solution of this salt? Atomic molar masss Ni = 58.7 g·mol-1
Set up the Gibbs energy equation (G) and calculate the Gibbs energy equation at 300 K and at 1300 K? At what temperature is the reaction spontaneous? hint: be very careful with the units of enthalpy and units of entropy.
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