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- what happens if temperature increases?
- Pressure decreased?
- More hydrogen added?
N2 +3H2 gives 2NH3
∆ H=-9.3.6 kJ
At equilibrium state for a reaction between Hydrogen and Iodine to give hydrogen at 675 k in 5 liter flask that contains 0.4 mole of hydrogen , 0.4 mole of iodine and 2.4 mole HI. calculate the equilibrium constant
Use atomic mass unit approach to determine the mass of 2.00*10^13 atoms of rubidium
Example of periodic table using hypothetical elements with pictures and explanation.
8. How many grams of CaCl2 will be dissolved in 50 kg of water at 70°C?
9. What amount of water is needed to dissolved 450g of Pb(NO3)2 at 40°C?
10. How many grams of water must be added to 35g of KNO3 to produce a saturated solution at 30°C?
Describe which of the following is unsaturated, saturated, or supersaturated? All solutions are prepared from 100 g of water.
a. 60 g KCL at 60°
b. 60 g K2Cr2O2 at 60°C
c. 60 g Pb(NO3)2 at 25°C
What mass of solute will dissolve in 100 g water at the following temperatures?
a. NaNO3 at 10°C
b. K2Cr2O7 at 30°C
c. NaCl at 50°C
Are these ionic, molecular, or mixture?
0.10 M acetic acid
0.0010 M hydrochloric acid
0.010 M hydrochloric acid
0.10 M hydrochloric acid
1.0 M hydrochloric acid
Prepare 100 mL of 0.200 bicarbonate buffer, pH 10 by calculating the mass of sodium bicarbonate and sodium carbonate.
a. Use the Henderson-Hasselbalch equation to calculate the volume of each stock
solution needed.
pH = pKa + log [conjugate base] / [weak acid]1
b. Check your calculations with other students. See the instructor if there is uncertainty.
c. Make the solution and check the pH of a portion of your buffer solution using the pH
meter.
L = 245μL
solution:
Preparation of Bicarbonate Buffer
Calculated Volume
CH3COOH ____________________
KH2PO4 ____________________
Actual pH of the buffer: ____________________
find the vapor pressure of a solution containing 35.0g calcium chloride (CaCl2) in 750.0g water. Note that the P water= 47.1 torr at 37.0C
