If 50mL of 0.1MHBr is mixed with 50mL0.2M,NaOH,find pH of resulting mixture
2.7
12.7
10.7
1.3

100 ml of 1M NaOH is mixed with 50ml of 1N KOH solution. Normality of mixture is

50.0 mL of 0.10 M HCl is mixed with 50.0 mL of 0.10 M NaOH. The solution's temperature rises by 3.0^(@)C . Calculate the enthalpy of neutralization per mole of HCl. (Assuming density of sol. =1 g//ml & specifice heat of water)

20 mL of 0.5 M HCl is mixed with 30 mL of 0.3 M HCl, the molarity of the resulting solution is :

100 ml of 0.1 N NaOH is mixed with 50 ml of 0.1 N H_2SO_4 . The pH of the resulting solution is

When 5.0 mL of a 1.0 M HCl solution is mixed with 5.0 mL of a 0.1 M NaOH solution, temperature of solution is increased by 2^@C predicted accurately from this observation?

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) )

6ml of 0.1M CH_(3)COOH when mixed with x ml of 0.1 M NaOH the pH of the resulting buffer solution was found to be 5.04 . The value of x is (log2=0.3)pK_(a(CH_(3)COOH))=4.74

100ml 0.1M H_(3)PO_(4) is mixed with 50ml of 0.1M NaOH. What is the pH of the resultant solution? (Successive dissociation constant of H_(3) PO_(4) "are" 10^(-3) , 10^(-8) and 10^(-12) respectively ?

If 100 ml of 0.1 M CH_3COOH and 200 ml of 0.03 M NaOH solutions are mixed together, then the pH of resulting mixture will be given [pk_a (CH_3COOH) = 4.74 and log 1.5 = 0.18)]

200ml of 1 M CH_(3)COOH(K_(a)=10^(-6)) is mixed with 200ml of 0.1M HCOOH(K_(a)=10^(-5)) . The pH of the resulting mixture is