1.70
pH = - log10 (2.1 x 10-6) = 5.68
11.9
3.2
3.2
HBr + NaOH ------> NaBr + H2O This is an acid-base reaction. The compounds will disassociate into ions in solution. The hydrogen from the HBr will go to the OH- and form water. The NaBr is a salt.
HBr + NH3 --> Br- + NH4+Ammonia is very well dissolved by acidic solution of hydrogen bromide being a gaseous base in acid solution.
Br2 + 2H2O + SO2 = H2SO4 + 2HBr
Hydrogen + Bromine ---> Hydgrone Bromide H + Br ---> HBr
The answer is 770,9 mL solution.
HBr + NaOH ------> NaBr + H2O This is an acid-base reaction. The compounds will disassociate into ions in solution. The hydrogen from the HBr will go to the OH- and form water. The NaBr is a salt.
HBr + NH3 --> Br- + NH4+Ammonia is very well dissolved by acidic solution of hydrogen bromide being a gaseous base in acid solution.
Br2 + 2H2O + SO2 = H2SO4 + 2HBr
Methane + Bromine --> Bromomethane + Hydrogen bromide
Hydrogen + Bromine ---> Hydgrone Bromide H + Br ---> HBr
The answer is 770,9 mL solution.
Al2O3 + 6HBr = 2Albr3 + 3H2O
I2 + 10 hno3 = 2 hio3 + 10 no2 + 4 h2o
HBr In a chemical equation you would write it as HBr(aq).
They are all 1: KOH + HBr = KBr + H2O
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
None. This is a metathesis reaction, and thus nothing is produced but a combination of the reactants (NH4Br, for example).