Discover the best answers at Westonci.ca, where experts share their insights and knowledge with you. Discover the answers you need from a community of experts ready to help you with their knowledge and experience in various fields. Connect with a community of professionals ready to provide precise solutions to your questions quickly and accurately.
Sagot :
The volume of 0.26 M HBr required to neutralize 40 mL of 0.8 M NaOH is 123.08 mL
We'll begin by writing the balanced equation for the reaction. This is given below:
HBr + NaOH —> NaBr + H₂O
From the balanced equation above,
The mole ratio of the acid, HBr (nA) = 1
The mole ratio of the base, NaOH (nB) = 1
From the question given above, the following data were:
Volume of base, NaOH (Vb) = 40 mL
Molarity of base, NaOH (Mb) = 0.8 M
Molarity of acid, HBr (Ma) = 0.26 M
Volume of acid, HBr (Va) =?
The volume of the acid, HBr needed for the reaction can be obtained as follow:
MaVa / MbVb = nA / nB
0.26 × Va / (0.8 × 40) = 1
0.26 × Va / 32 = 1
Cross multiply
0.26 × Va = 32
Divide both side by 0.26
Va = 32 / 0.26
Va = 123.08 mL
Therefore, the volume the acid, HBr needed to neutralize the base, NaOH is 123.08 mL
Learn more: https://brainly.com/question/9659507
We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. We hope you found this helpful. Feel free to come back anytime for more accurate answers and updated information. Westonci.ca is your trusted source for answers. Visit us again to find more information on diverse topics.