if 10ml of 0.1M A neutralize 50ml of 0.05M`(OH)_2` Find the basicity of A

0.45 g of acid (mol. Wt. =90 ) was exactly neutralized by 20 ml of 0.5(M) NaOH . The basicity of the given acid is

If 50 ml of 0.1 M NaCl and 50 ml of 0.1 M BaCl_(2) are mixed, molarity of chloride ion in the resulting solution will be

If 50ml of 0.2 M KOH is added to 40 ml of 0.05 M HCOOH , the pH of the resulting solution is ( K_(a)=1.8xx10^(-4) )

100 ml of 0.15 M HCl is mixed with 100 ml of 0.05 M HCl, is the pH of the resulting solution?

What is the "pH" of "100ml" of 0.1MHCl + 300ml of 0.1M H_(2)SO_(4) + 100ml of 0.3M Ba(OH)_(2) and volume was made to "1L" by a

Calculate the pH of each of the following solution (i) 100 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. (ii) 100 ml of 0.1 M CH_(3)COOH mixed with 50 ml of 0.1 m NaOH (iii) 50 ml of 0.1 M CH_(3)COOH mixed with 100 ml of 0.1 M NaOH. K_(a)(CH_(3)COOH)=1.8xx10^(-5)

10ml of 0.1M weak acid HA(K_(a) = 10^(-5)) is mixed with 10 ml 0.2 M HCI and 10ml 0.1 M NaOH . Find the concentration of A^(-) in the resulting solution. Write your answer as (-log [A^(-)])

What is the molarity of a hydorchlric acid solution if 20.00 mL of it neutralizes 18.46 mL of a 0.0420M Ba(OH)_(2) solution?