Consider the reaction of 50.7 mL of 0.310 M NaC₇H₅O₂ with 50.0 mL of 0.245 M HBr. (Ka of HC₇H₅O₂ = 6.3 x 10⁻⁵) Write the net ionic equation for the reaction that takes place. What would the general form look like in terms of H2O, H+,H3O+,H, O, OH-, and C?

A 0.251 g sample of impure NaOH requires 17.6 mL of 0.2903 M HCl for neutralization. What is the percent of NaOH in the sample, by weight?

A 0.212 g sample of impure NaOH requires 18.2 mL of 0.2879 M HCl for neutralization. What is the percent of NaOH in the sample, by weight? % NaOH=

Consider the reaction of 66.5 mL of 0.310 M NaC₇H₅O₂ with 50.0 mL of 0.245 M HBr. (Ka of HC₇H₅O₂ = 6.3 x 10⁻⁵) a)Write the net ionic equation for the reaction that takes place. (In terms of C, H2O, H3O+, O, H, H+, OH-) b) How many moles of C7H5O2- would be present before the reaction takes place? c) How many moles of H+ would be present before the reaction takes place? d)What species would be left in the beaker after the reaction goes to completion? e) How many moles of C7H5O2- would be left in the beaker after the reaction goes to completion? f) How many moles of HC7H5O2 would have been produced after the reaction goes to completion? g) What would be the pH of this soultion after the reaction goes to completion?

What is the pH of a solution of 0.160 M nitrous acid(HN02; Ka=4.0 x10^-4)

i.e. Determine the [H+] of a 500.0 mL solution that contains2.6 g of NaOH

Complete and balance the following neutralization reaction: NaOH(aq)  +  HC2H3O2(aq) --> What are the products of this reaction before balancing?

If the ph of a 30.0 mL sample of 1.0 M NaOAc is 9.33, what's the equilibrium [H+] and the Ka value?

10g of the strong base Ba(OH)2 is dissolved in 200 mL of water and then titrated with 0.100 M HCl. How many mL of the acid solution must be added to exactly neutralize the solution?

What volume of H2SO4 of concentration 0.04 M is required to completely neutralize 200 mL of Al(OH)3 of concentration 0.02 M.