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Control test tube A contains 1mL each of solutions of BiCl3 and NH3. Test tube B contains 1mL each of solutions of BiCl3 and NH3 and 1g of NH4Cl. A clear gelatinous precipitate of Bi(OH)3 forms in test tube A while no ppt. forms in test tube B. The appearances of test tubes A and B are due to the interplay between the ammonia and bismuth hydroxide equilibria. NH3(aq) + H2O(l) <--> NH4+(aq) + OH-(aq) Bi+3(aq) + 3OH-(aq) <--> Bi(OH)3(s) What common ion is present in test tube B? How does addition of this common ion affect the ammonia and hismuth hydroxide equilibria? Explain the results (difference in appearance between test tubes A and B) in terms of the common ion effect. What will happen in test tube A if concentrated HCl is slowly added? Explain.
Based on the following values, the value for Delta S for the decomposition of one mole of gaseous sulfur trioxide to give solid sulfur and oxygen gas is: S(s): S = 31.88 O2(g): S = 205.0 SO3(g): S = 256.2
Aluminum chlorhydrate is added to antiperspirants to stop people from sweating. If this compound contains neutral H2O molecules and Al3+, OH- and Cl- ions, and the formula of this compound is Alx(OH)5Cl 2H2O, what is the value of x in this formula
500cm3 of 0.250M of Na2SO4 is added to an aqueous solution of 15.0g of BaCl2 resulting in a white precipitate of insoluble BaSO4.
What is the percent hydrogen (H) by weight of a solution containing 53.5mL of CH3COCH3? The density of acetone is 0.788 g/mL
hard, amorphous polymers become soft and flexible at the glass transition temperature B) crystalline regions of a polymer melt transition temperature C
A copper wire with a mass of 4.32 g reacts with sulfur to form 5.41 g of a copper sulfide compound. a) Determine the number of moles of copper and sulfur in the compound. b) Determine the empirical formula of the product.
A 50.0 L steel vessel, filled with CH4 to a pressure of 10.0 atm at 298 K, is heated to 1600 K to convert CH4 into C2H2 . What mass of C2H2can be produced. What pressure does the reactor reach at 1600 K? 2CH4 (g) C2H2(g) + 3H2(g)
Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 765 mmHg and a temperature of 35*C.
What mass of sucrose should be combined with 454 g of water to make a solution with an osmotic pressure of 8.85 atm at 285 K
Pure solid NaH2PO4 is dissolved in distilled water, making 100.0ml of solution. 10 ml of this solution is diluted to 100.00 ml to prepare the orignal phosphare standard solution
Amount of H2O2 in 15.8 g of hair bleach was obtained by titration with a standard KMnO4 soln.
at 710. mm hg a sample of nitrogen gas occupies 625 ml what volume does the gas occupy if the temperature constant and the pressure increases to 760. mm hg
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