You are to make 10.0 L of 1.20 M Potassium nitrate solution. What molarity would the potassium nitrate solution need to be if you were to use only 2.50 L of it?

a) molarity = moles / volume Molarity = 0.150/1.10 = 0.136Mb) moles = 32.9/56.38 = 0.583molesVolume = 763ml = 0.763LMolarity = moles / volume Molarity = 0.583/0.763 = 0.764 M

Reaction:Au3+ + Fe = Fe3+ + AuV(Au(NO3)3 solution) = 2.8x1023/(6.02x1023)/0.5 = 0.93 LAnswer: 0.93 L

M=mol/volume Volume=mol/MV= 0.021÷0.5 = 0.042 LVolume in Ml = 0.042×1000Ans= 42mL

Gold nitrate solution volume =0.93L

KH2PO4 + HNO3 → H3PO4 + KNO3According to the reaction equation:n(KH2PO4)=n(KNO3) = 119 mol

Solutions of known concentration can be prepared either by dissolving a known mass of solute in a solvent and diluting to a desired final volume or by diluting the appropriate volume...

СM = n/V n = m/M M (KNO3) = 101 g/mol n (KNO3) = СM x V = 0.75 x 10 = 7.5 mol m (KNO3) = n x M =...

Solution:Molarity = mol solute / solution volumeHence,Moles of NH4NO3 = Molarity × Solution volume = 2.50 M × 0.15 L = 0.375 molMoles = Mass / Molar massThe molar mass...

Answer:2HNO3 = 2HNO2 + O2m= 85 x 0.1235 / 69= 0.1521W%= 0.1521 / 0.4230 = 36%

aluminum nitrate