It turns out that Ba(OH)2 is also considered a strong base. What is the [OH-] concentration in 0.34 M Ba(OH)2(aq) solution?

what volume in mL of 0.026 M HBr solution is to be required to titrate 125mL of a 0.032 M NaOH solution? NaOH(aq) + HBr(aq) -> NaBr(aq) + H2O(I)

Aluminum sulfate, known as cake alum, has a remarkably wide range of uses, from dyeing leather and cloth to purifying sewage. In aqueous solution, it reacts with base to form a white precipitate. (a) Write balanced total and net ionic equations for its reaction with aqueous NaOH. (Type your answer using the format (NH4)2CO3 for (NH4)2CO3, [NH4]+ for NH4+, and [Ni(CN)4]2- for Ni(CN)42-. Use the lowest possible coefficients. Type the cation before the anion.)overall equation  (aq) +  NaOH(aq)    (aq) +   (s)net ionic  (aq) +   (aq)    (s)(b) What mass of precipitate forms when 104.5 mL of 0.616 M NaOH is added to 517 mL of a solution that contains 18.4 g aluminum sulfate per liter?  g

Write the balanced net ionic equation including heat in the equation. The reaction is exothermic.

By titration, it is found that 55.5 mL of 0.116 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution. [HCI] M

By titration it is found that 35.7 mL of 0.101 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.

What is the answer?

What is the difference between a strong acid such as hydrochloric acid, HCl(aq), and a weak acid such as acetic acid, HC2H3O2(aq)?

If you begin with 28.4 mL of 0.287 M HCl(aq) solution and mix it with 17.3 mL of 0.181 M NaOH(aq), what is the final pH when they are mixed together?HCl(aq)+ NaOH(aq)→ H2O(l) + NaCl(aq)

In the following acid-base titration experiment NaOH(aq) + HNO3(aq) ———> NaNO3(aq) + H2O(1). What is the molarity of the HNO3 solution if 18.3 mL of 0.115 M NaOH was used to neutralize 25 mL of HNO3? (a) 0.157 M (b) 0.0842 M (c) 3.978 M (d) 0.0157 M