Hi,
I need a hand on the following:
1. 25.00mL of a 0.100M solution of Hal is added to 25.00mL of a 0.180M solution of NaOH. What is the concentration of OH^- (aq) in mol L^-1, remaining in the solution?
(A) 0.0400
(B) 0.0500
(C) 0.0800
(D) 0.1000
2. 50.00mL of a 0.020M solution of Ba(OH)2 is added to 50.00mL of a 0.060M of HNO3. The hydrogen ion concentration in the resultant solution, in mole per litre, is-
(A) 0.010
(B) 0.020
(C) 0.030
(D) 0.040
3. 0.132g of a pure carboxylic acid (R-COOH) was dissolved in 25.00mL of water and titrated with 0.120 mol L^-1 of standardised NaOH solution. A volume of 14.80 mL was required to reach the endpoint of titration. Identify the carboxylic acid.
Thanks!!!
I need a hand on the following:
1. 25.00mL of a 0.100M solution of Hal is added to 25.00mL of a 0.180M solution of NaOH. What is the concentration of OH^- (aq) in mol L^-1, remaining in the solution?
(A) 0.0400
(B) 0.0500
(C) 0.0800
(D) 0.1000
2. 50.00mL of a 0.020M solution of Ba(OH)2 is added to 50.00mL of a 0.060M of HNO3. The hydrogen ion concentration in the resultant solution, in mole per litre, is-
(A) 0.010
(B) 0.020
(C) 0.030
(D) 0.040
3. 0.132g of a pure carboxylic acid (R-COOH) was dissolved in 25.00mL of water and titrated with 0.120 mol L^-1 of standardised NaOH solution. A volume of 14.80 mL was required to reach the endpoint of titration. Identify the carboxylic acid.
Thanks!!!