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Molarity and Solubility
1) If ZnCO3 (solid) is insoluble in water, but dissolves in excess 6.0 molar HCl (aqueous), how would pull out the proper equation that would support it?
2) How would you go about finding how many mL of 2.00 molar NaOH (Aqueous) solution are required to neutralize 1.858 g of KHC8H4O4 (it's formula weight being 204.22)? Any other example would do.
NaOH(aq) + KHC8H4O4 --> NaKC8H4O4(aq) + H2O(l)
3) Potassium nitrate, KNO3, has a formula weight of 101.10. How would I find the molar concentration of a solution prepared by dissolving 7.58 grams of potassium nitrate in enough water to prepare 250 mL of the solution?
Light with a frequency of 7.11 x 10 -14 Hz lies in the violet region of the visible spectrum. What is the wavelength of this frequency of light? Answer in units of nm.
Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen: 4KNO3(s)→ 2K2O(s) + 2N2(g) + 5O2(g)
You are given the following data. S(s) + 3/2 O2(g) → SO3(g) ΔH = -395.2 kJ 2 SO2(g) + O2(g) → 2 SO3(g) ΔH = -198.2 kJ Calculate ΔH
A solution contained KIO3 and excess KI. 25 cm3 of this solution were acidified and the liberated I2 required 26.8 cm3 of 0.1 M Na2S2O3 for complete recaction.
A commercial plant is to treat 320 m3/hr of feed consisting of 50 % A, 50% inerts at 25 atm and 350ºC to obtain eighty percent conversion. Determine how many 2-m lengths of 2.5 cm ID pipe are required?
A sample containing 0.187 g Cl- is dissolved in 50.0 mL water.How many moles of Cl- ion are in the solution?What is the molarity of Cl- ion in the solution.
how many milliliters of a stock solution of 2.00 m kno3 would you need to prepare 100.0 ml of 0.150M KNO3
the temperature of a 4.00L sample of gas is changed from 10.0c to 20.0c. what will the volume of this gas be at the new temperature if the pressure is held constant?
When 3.00 g KNO3 are dissolved in 50 g glycerol, the freezing point changes from 17.8°C to 13.6°C. What is the freezing point depression constant (Kf ) for glycerol.
pH = log[H3O+] , pH + pOH = 14, [H3O+] * [OH-] = 1.0 X 10^-14, pH = -log(0.001) = 3 Could you show me a few of the steps between line one and two in both of these conclusions?
Calculate the mass of one oxygen atom and determine the number of oxygen atoms in a 10.00g sample of the element.
If 200 mL of 0.300 M Cr(NO3)3(aq) is added to 100 mL of 4.0 × 10^-4 M NaF(aq) at 25 degrees celcius, will a CrF3 precipitate form? For CrF3 in water at 25°C, Ksp = 6.6 × 10^-11.
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