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1. Write balanced net ionic equation for the first stage of dissociation of the triprotic acid H3PO4.
2. Write balanced net ionic equation for the second stage of dissociation of the triprotic acid H3PO4.
3. Write balanced net ionic equation for the third stage of dissociation of the triprotic acid H3PO4
4. The concentration of CH3NH3+ in a 0.20 M methylamine (CH3NH2) solution is 2.32 × 10-6 M. What is Kb for methylamine?
5. Calculate the concentrations of all species present in 0.29 M NH3 (Kb=1.8×10-5).
6. Calculate the pH of the hydrated cation in Fe(NO3)3 (Ka=6.3×10-3).
7. Calculate the percent dissociation of the hydrated cation in Fe(NO3)3 (Ka=6.3×10-3).
0.22 litre of an idealmonatomic gas cv 3r2 initially at 12 deg c and 1.7 atmpressure undergo an expansion against a
A plant must absorb 48 moles of photons with a wavelength of 430 nm for every mole of sugar that it produces. If a plant absorbs 36.5 moles of photons with a wavelength of 430. nm, how much energy in kJ has it absorbed
HCL acid solution is standardized using 0.502g of sodium carbonate. Find the molarity of the acid if 30.5mL are required for the titration.
Write a balanced chemical equation for the reaction between CN - and MnO4- in basic solution. The skeleton ionic reaction is given below.
For the microscale titration between KMnO4 and H2O2 the balanced net ionic equation is 2 MnO4-(aq) + 5 H2O2(aq) + 6 H+(aq) --> 2 Mn2+(aq) + 5 O2(g) + 8 H2O(l)
A) Draw the major organic product obtained when 1,2-dimethylcyclohexane-1,2-diol encounters periodic acid.
A gas-filled balloon having a volume of 2.50 L at 1.2 bar and 25°C is allowed to rise to the stratosphere (about 30 km above the surface of Earth), where the temperature and pressure are -23°C and 3.00 10-3 atm, respectively. Calculate the final v..
compute the water volume that is released upon its total metabolism to carbon dioxide and H 2 O, taking into account any oxidative phosphorylation that might occur.
A 32.0-g sample of water at 260. K is mixed with 47.0 g water at 300. K. Calculate the final temperature of the mixture assuming no heat loss to the surroundings.
Compute the change in internal energy delta e for a system that is absorbing 35.8 kJ of heat as well as is expanding from 8.00 to 24.0 L in volume at 1.00 atm. Remember that 101.3 J= 1 l*atm.
What is the change in E for the reaction in kJ/mol of C7H8. The heat capacity of the calorimeter was 780 J/Celsius. The specific heat of water is 4.184 J/gCelusius.
Hydrocarbon mixtures are used as fuels. What mass of CO2 gas is produced by the combustion of 189.2 g of a mixture that is 57.6 % CH4 and 42.4% C3H8 by mass
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