In 100 ml, mole of NH4OH is 0.7133
So in 1ml, mol of NH4OH is (0.7133/100) = 7.133* 10-03
what is the mol of ammonia in a 25%ammonia solution that is NH4OH? g/mol: 35,05 and g/ml: 1 mL ( consider density)
28. A concentrated ammonia solution has a density of 0.900 g/mL at 25°C and is 14.8 M. What is the percent by mass of NH3 in the solution? a. 28.0% NH3 by mass b. 18.9% NH3 by mass c. 0.6% NHz by mass d. 9.7% NH3 by mass e. 1.6% NH3 by mass wal. 1 2
You need to prepare 200 mL of a 0.4 M solution of ammonium hydroxide (NH4OH) You have 80 mL of a 0.5 M NHOH solution and 40 mL of a 7.5% (w/v) NH4OH solution. What volume of 7.5% NHOH and water needs to be added to the 80 mL of 0.5 M NH4OH solution to make up 200 mL of 0.4 M NH4OH? Molar mass of NH4OH 35.04 g/mol % (weight / volume) means mass (in g) in volume (100...
An aqueous solution is 0.500% by mass ammonia, NH3, and has a density of 0.996 g/mL. The molality of ammonia in the solution is m.
A 3.82 L volume of gaseous ammonia, NH3 (g), at STP is bubbled through 100.0 mL water and reacts completely to form ammonium hydroxide, NH4OH (aq). a) What is the molar concentration of the resulting NH4OH (aq) solution? b) What mass of NH4OH is present in the 100.0 mL solution? c) How many moles of NH4OH would be present in 482 mL of a solution of the same concentration?
The density of a 0.84 M aqueous sugar (C12H22O11) solution is 1.12 g/mL at 25°C. What is the molal concentration? The molar mass of C12H22O11 = 342.3 g/mol.
A solution of household ammonia is 3.0 % NH3(aq) and has a density of .98 g/ml. What is the molar concentration of the NH3(aq)? Given that the Kb for NH3(aq) = 1.8x10‒5, what is the predicted pH of this solution? Thank you in advance
What is the molarity of 38.25 g of NH4OH dissolved to make 525 mL solution? TT T Arial 3 (12pt) T- ABC MI i
The density of a 0.84 M aqueous sugar (C12H22O11) solution is 1.12 g/mL at 25°C. What is the molality? The molar mass of C12H22O11 = 342.3 g/mol. Dinitrogen tetroxide decomposes to produce nitrogen dioxide: N2O4 (g) ↔ 2 NO2 (g) Calculate the equilibrium constant for the reaction given the equilibrium concentrations at 100°C: [N2O4] = 0.800 M and [NO2] = 0.400 M
A solution of NaCl (MW = 58.5 g/mol) in water (MW = 18.0 g/mol) has the molality of 3.01 molal and the density of 1.112 g/mL. Consider mass of solvent 1 Kg A) What is the mass percent of the solute? (B) What is the molarity of the solution? (C)What is the mole fraction of H2O?
An solution of antifreeze is prepared by mixing 21.0mL of ethylene glycol (d = 1.11 g/mL; molar mass = 62.07 g/mol) with 50.0 mL H2O (d = 1.00 g/mL) at 25°C. If the density of the antifreeze solution is 1.07 g/mL, what is its molarity?