0
The reaction is:
HBr + KOH = KBr + H2O
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What is the concentration of a HBr if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
0.75 M
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
What salt forms when you combine HBr and KOH?
KBr and some water H2O
What are the numbers for equation koh hbr equals kbr h2o?
They are all 1: KOH + HBr = KBr + H2O
Is KOH HCI H2O a balanced equation?
NO!!! It is a neutralisation reaction. Reason it produces water (pH =7) KOH + HBr = KBr + H2O KBr (Potassium bromide) is a (chemical) salt. Remember the the empirical acid equations. Acid + Alkali = Salt + water Acid + Base = Salt + water Acid + metal = Salt + hydrogen Acid + carbonate = Salt + Water + Carbon dioxide. NB Acid formulas are always writen as 'HA'. Where 'A' is the anion. Alkali formulkas are always written as 'MOH'. Where 'M' is the metal cation. NNB Notice the positions of the 'H' in these formulas.
What is the concentration of a HBr if 12.0 mL of the solution is neutralized by 15.0 mL of a 0.25 M KOH solution?
0.75 M
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
What salt forms when you combine HBr and KOH?
KBr and some water H2O
What are the numbers for equation koh hbr equals kbr h2o?
They are all 1: KOH + HBr = KBr + H2O
Is KOH HCI H2O a balanced equation?
NO!!! It is a neutralisation reaction. Reason it produces water (pH =7) KOH + HBr = KBr + H2O KBr (Potassium bromide) is a (chemical) salt. Remember the the empirical acid equations. Acid + Alkali = Salt + water Acid + Base = Salt + water Acid + metal = Salt + hydrogen Acid + carbonate = Salt + Water + Carbon dioxide. NB Acid formulas are always writen as 'HA'. Where 'A' is the anion. Alkali formulkas are always written as 'MOH'. Where 'M' is the metal cation. NNB Notice the positions of the 'H' in these formulas.
A 76.0ml volume of 0.25m HBr is titrated with 0.50m KOH calculate the pH after addition of 38.0ml of KOH?
76.0*0.25=19 38.0*0.50=19 19-19=0 Cancel each other out ANSWER=7 just water and salt(not acid <7)(not basic >7)
A 10.0 ml of 0.121 m h2so4 is neutralized by 17.1 ml of koh solution the molarity of the koh soultion is?
M1V1=M2V210mLX0.121 = ? X 17mL=0.0708
What are the acid and the base that were neutralized to produce KCl?
KOH - potassium hydroxide or caustic potash and HCl hydrochloric Acid
Balanced molecular equation of Aqueous acetic acid is neutralized by aqueous potassium hydroxide?
CH3COOH + KOH = CH3COOK + H2O
What is formed when HCl reacts with KOH?
KCl and water are formed.
Is Cu2SO4 a strong acid?
It's a salt with a high pH.Strong acids Weak acidsWeak bases Strong bases HBr CH3COOH NH3 NaOH HCl HF NH4OH KOH H2SO4 HCN Cu(OH)2 Ca(OH)2
If 25.0 ml of 1.48m h2so4 can be neutralized with 27.29 ml of koh what is the molarity of the koh?
25 milliliters of the solution has . 037 moles of H2SO4. The neutralization reaction is H2SO4 + 2 KOH yields 2 H2O + K2SO4. So, . 074 moles of KOH are required. This equals 2. 71 mL of solution.
