I really need to know the answers to these questions by tomorrow, if anyone can show me how to do them I would be eternally grateful!
1. Calculate the pH of a 5.0 M H3PO4 solution at 25 given that the equilibrium constants are 7.5x10^-3 , 6.2x10^-8 , and 4.8x10^-13 for the first, second and third ionisation reactions respectively.
2. A solution is made by dissolving 0.1mol of HCN gas and 0.1mol of HCl gas in 1L of water. What is the concentration of CN- in the solution if the ionisation constant for HCN is 6.2x10^-10?
3. A workable electrochemical cell comprises a Pb/Pb2+ half cell connected to a Mg/Mg2+ half cell. Identify the balanced equation for the cell reaction, the material present in each half cell, the regions where oxidation and education occur, the anode/cathode and reactions at each, the direction of electron flow/movement of negative ions through the cell and positive/negative electrodes.
4. Complete and balance (you may assume these reactions occur in aqueous acid solution)
- Fe3+ + Mg -> Mg2+ + Fe
- I2 + S2O3 2- -> I- + SO2
Also, are these statements true?
- CBr2CCl2 is a polar molecular that contains polar and non-polar bonds
- Fe is a weaker oxidising agent than Sn2+
- Br- can be oxidised by Sn2+
- When the volume of gas decreases, the pressure increases but the temperature and moles of gas stay the same
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