JUNDY

Most popular questions and responses by JUNDY
  1. Chemistry

    A solid weak acid is weighed, dissolved in water and diluted to exactly 50.00 ml. 25.00 ml of the solution is taken out and is titrated to a neutral endpoint with 0.10 M NaOH. The titrated portion is then mixed with the remaining untitrated portion and the

    asked on April 14, 2015
  2. Chemistry

    A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The

    asked on February 25, 2015
  3. Chemistry

    Calculate Keq for 2 moles of electron(s) in each half-reaction and a standard potential of 0.55 V.

    asked on April 12, 2015
  4. Chemistry

    Calculate ΔG (in kJ) at 298 K for some solid ZnF2, 0.055 M Zn2+ and 0.063 M F-(aq). I found Q to be 2.18e-4, then i implemented it into the equation deltaG=RT(lnQ). I got -20.89, but the answer is -12.2.

    asked on April 7, 2015
  5. Chemistry

    Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 70 mL of the concentrated HCl, adding it to water, and diluting to 0.500 L. Calculate the approximate molarity of this solution from the

    asked on March 15, 2015
  6. Chemistry

    What is the oxidation state assigned to Cr in zinc dichromate, ZnCr2O7?

    asked on April 12, 2015
  7. Chemistry

    Calculate ΔGo (in J) for 2 moles of electron(s) in each half-reaction and a standard potential of 0.57 V.

    asked on April 12, 2015
  8. Chemistry

    Calculate the average C—C bond strength in cyclopropane (in kJ/mol). Its combustion and the experimental enthalpy of reaction are: C3H6(g) + 4.5O2(g) → 3CO2(g) + 3H2O(g) ΔHºrxn = -1,957.7 kJ/mol Since all reactants and products are in the gaseous

    asked on April 7, 2015
  9. Chemistry

    1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*

    asked on March 10, 2015
  10. Chemistry

    The autodissociation of water to H+ and OH- is endothermic. At a higher temperature more of the water molecules have sufficient energy to dissociate. So, Kw is greater. At 25oC, Kw = 1.0 x 10-14. (standard Kw) At 65oC, Kw = 1.0 x 10-13. Calculate the

    asked on February 27, 2015
  11. Chemistry

    A reaction at 3.24 atm consumes 5.10 L of a gas adiabatically (q = 0). Calculate the change in internal energy of the system (in kJ).

    asked on March 31, 2015
  12. Chemistry

    There are three isotopes of phosphorus. Only one of them is stable. Calculate the binding energy per nucleon (in MeV) for P-32 (atomic mass = 31.9739 u). mass H = 1.007825 u and mass n = 1.008665 u. I multiplied the protons(15) by the mass H, and the

    asked on April 30, 2015
  13. Chemistry

    1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*

    asked on March 10, 2015
  14. Chemistry

    Calculate the hydrogen ion concentration, [H+], in 0.00988 M Ba(OH)2. Careful!

    asked on February 27, 2015
  15. Chemistry

    A reaction at 3.24 atm consumes 5.10 L of a gas adiabatically (q = 0). Calculate the change in internal energy of the system (in kJ). I know that I have to use w=-p deltaV but how do i find the Final and Initial volumes?

    asked on March 31, 2015
  16. Chemistry

    1)A buffer solution that is 0.10 M sodium acetate and 0.20 M acetic acid is prepared. Calculate the initial pH of this solution. The Ka for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. *A buffered solution resists a change in pH.*

    asked on March 10, 2015
  17. Chemistry

    1.578 g of an unknown hydrocarbon (110.7 g/mol) burns in bomb calorimeter in excess oxygen. The heat capacity of the calorimeter,Cv, = 5.709 kJ/ºC and ΔT =7.995 ºC. Find ΔE for this hydrocarbon in kJ/mol.

    asked on March 31, 2015
  18. Chemistry

    A reaction at 2.43 atm produces 20.0 L of a gas and evolves 75.3 kJ of heat (exothermic). Calculate the change in internal energy of the system (in kJ).

    asked on March 31, 2015
  19. Chemistry DrBob please answer

    A reaction at 3.24 atm consumes 5.10 L of a gas adiabatically (q = 0). Calculate the change in internal energy of the system (in kJ). I know that I have to use w=-p deltaV but how do i find the Final and Initial volumes?

    asked on March 31, 2015
  20. Chemistry

    A half-cell that consists of a copper wire in 1.00 M CuNO3 solution is connected by a salt bridge to a half cell containing a 1.00 M X(II) acetate solution and an electrode of metal X. The voltage of the cell is 2.00 V, with metal X as the positive

    asked on April 12, 2015
  21. Chemistry

    Calculate the vapor pressure of Hg at 14 oC (in atm). Hg(l) ↔ Hg(g) . . . ΔHo = 61.32 kJ and ΔSo = 98.83 J/K

    asked on April 7, 2015
  22. Chemistry

    Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. The Ka for HOCl is 3.0 x 10-8 M. What is the pH when half the acid has been neutralized? 'I got 7.82 by using the HH formula but its wrong, help.

    asked on March 15, 2015
  23. Chemistry

    Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. The Ka for HOCl is 3.0 x 10-8 M. What is the pH at the equivalence point? I used the HH formula and got pH=7.52+log(.222)=6.87, but its not right.

    asked on March 15, 2015
  24. Chemistry

    Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. The Ka for HOCl is 3.0 x 10-8 M. What is the pH when half the acid has been neutralized? 'I got 7.82 by using the HH formula but its wrong, help.

    asked on March 15, 2015
  25. Chemistry

    Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. The Ka for HOCl is 3.0 x 10-8 M. What is the pH at the equivalence point? I used the HH formula and got pH=7.52+log(.222)=6.87, but its not right.

    asked on March 15, 2015
  1. Math

    y=(3/2)^x

    posted on April 14, 2015
  2. math

    Yes, that's correct.

    posted on April 14, 2015
  3. Chemistry

    It's a limiting reagent problem. 8mol*(64.07 g/mol)=512.56 g 16mol*(34.07 g/mol)=545.12 g Therefore, SO2 is the limiting reagent. Figure out the rest

    posted on April 14, 2015
  4. MATH

    In an arithmetic series, every term is separated from its neighbours by the same difference. So given an arithmetic sequence that starts with the first value A and has a common difference of D, the first five terms are: 1st term: A 2nd term: A + D 3rd

    posted on April 14, 2015
  5. Chemistry

    Don't Include Oxygen in your equation and try it again.

    posted on April 14, 2015
  6. chemistry

    M1V1 = M2V2 (.125L)(10.30M)=(x)(.500M)

    posted on April 14, 2015
  7. Statistics

    a. 3/4 b. 4/8 c. 1/4 d. 2/7

    posted on April 12, 2015
  8. biology

    Google it bro

    posted on April 12, 2015
  9. math

    Just multiply all three dimensions to get you volume.

    posted on April 12, 2015
  10. Chemistry

    Actually can you help me find the pH at the equilibrium point, my work: HOCl OH- I .004 .004 C -.004 -.004 E 0 0 .01*.400=.004 .008*.5=.004 I don't know what to do next...

    posted on March 15, 2015
  11. Chemistry

    Ill post my work

    posted on March 15, 2015
  12. chemistry

    Find the moles of ethanol and the moles of the solution, and divide ethanol by the solution.

    posted on March 15, 2015