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The following electron configurations correspond to neutral atoms in excited states. What is the element and what is the ground state electron configuration for each atom?
1. 1s2 2s2 2p6 3s2 3p6 3d5
2. [Kr] 5s2 4d10 5p4 6s1
a 5.96-g sample of homogentisic acid a weak organic acid having ka4.0 x 10-5 is dissolved in 35.0 ml of water and its
If you have 100 ml of pure water and add to it 100 ml of 2.0M HC2H3O2. What will be the final solution pH
You need to make 500 ml of 100 mM potassium phosphate buffer at pH 7.5. You have the stock solutions of KH2PO4 and K2HPO4 at 1M each. You will make the buffer by adding some of each of these stock solutions to water.
Chester makes 1 L of a 0.01 M HCL solution and measure the pH. Burt then adds 5.80 g of sodium chloride to Chester's solution and measures the pH. Compute the difference between the two pH values obtained.
Which of the following ionic compounds would be predicted to have the greatest (most negative) lattice energy. A. KBr
If 25.0 mL of 0.451 M HNO3 solution is titrated with 0.451 M NaOH, Calculate the pH of the solution after each of the following amounts of base have been added. Set up the relevant neutralization reaction equations for each part.
What is the wavelength (in nanometers) associated with a photon which has an energy content of 4.86E-24 kJ
What Volume of .0200 M KMNO4 is required to titrate a solution containing
Problem- The standard free energy change for the hydrolysis of ATP is -30.5 kJ. In a particular cell, the concentrations of ATP, ADP, and Pi are 3.2×10?3M , 1.1×10?3M , and 4.7×10?3M , respectively Calculate the free energy change for the hydrolys..
Describe the bonding in SeO2 in valence bond terms. Note whether or not there is delocalized bonding and explain how molecular orbital theory can be useful here.
Calculate the [CH3CO2H] ionized in solution for 0.1M acetic acid knowing that ph= 2.9 [H+]= 1.26 x 10^-3 M , [OH-]= 7.94 x 10^-12 M
For the reaction A(aq) + 2B(aq) 3C(aq) + D(aq) at 25oC and each substance at 0.1 M concentration, G was found to be 115 kJ. Explain which direction must the reaction proceed to reach equilibrium
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