How many molecules are in 3.21 moles of HBr?
3.21 moles HBr (6.022 X 10^23/1mole HBr)
= 1.93 X 10^24 molecules of HBr
What is the concentration of a HBr solution in 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
Balanced equation. KOH + HBr -> KBr + H2O everything is one to one, so... Molarity = moles of solute/liters of solution ( change ml to liters ) 0.25 M KOH = moles KOH/0.015 liters = 0.00375 moles of KOH this is as many moles that you have of HBr, so... Molarity of HBr = 0.00375 moles/0.012 liters = a concentration of HBr that is 0.31 M
How many grams of solid sodium hydroxide would need to be added to completely neutralize 35.0 mL of 1.45 M HBr?
This is a titration question: we want to have the same number of hydroxide ions as hydroxide ions so that they will form water and the pH will be neutral. In chemistry, we count atoms and molecules in moles, and we can calculate how many moles of HBr we have, because concentration in molarity is the number of moles divided by the volume in liters... M = moles/V. We plug in what we got: 1.45M…
What volume of a 0.394 M hydrobromic acid solution is required to neutralize 29.2 mL of a 0.140 M sodium hydroxide solution?
HBr + NaOH ------> NaBr + H2O so it is a 1:1 molar reaction. 29.2/1000 x 0.140 = 0.004088 moles of sodium hydroxide present and thus the same number of moles of HBr required. There are 0.394/1000 = 0.000394 moles per mL of HBr and thus 0.004088/0.000394 = 10.38 mL (2 decimal places) of HBr required for neutralization.
How many grams HBr are required to produce 150g AlBr3 in the equation 2Al plus 6HBr producing 2AlBr3 and 3H2?
Given the balanced equation 2Al + 6HBr --> 2AlBr3 + 3H2 In order to find how many grams of HBr are required to produce 150g AlBr3, we must convert from mass to mass (mass --> mass conversion). 150g AlBr3 * 1 mol AlBr3 * 6 molecules HBr = 136.52 or 137g HBr ----------- 266.6g AlBr3 * 2 molecules AlBr3
How many moles of ammonium bromide can be produced from 250 moles of bromine and 600 moles of ammonia?
This is to do with the intermolecular forces in the two compounds. There are no hydrogen bonds between the molecules of either compound, since Br and I are not electronegative enough to polarise the molecules sufficiently. But since HI molecules contain more electrons than HBr, there are increased van der Waals forces in HI. For the same reason HBr has a higher boiling point than HCl, but HF has a higher boiling point than HCl…