24. A buffer is prepared using acetic acid, CH3COOH, (a weak acid) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions:   Volume of CH3COOH(aq):   135.0 mL Concentration of CH3COOH(aq):  1.014 M   Volume of CH3COONa(aq):  123.0 mL Concentration of CH3COONa(aq):  1.204 M   What is the concentration of the conjugate base, CH3COO-, component in the final buffer solution? Give your answer in M, with correct significant digits.

Consider the following acid-base reaction:HClO4(aq) + KOH(aq) -> KClO4(aq) + H2O(l)How many millilitres of a 2.00 M potassium hydroxide solution is required to titrate25.0 millilitres of a 1.45 M solution of perchloric acid

Complete the balanced molecular reaction for the following weak base with a strong acid: NaClO2(aq) +H2SO4(aq) ->

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please write the neutralization equation by explaining it ; "Identify acids and bases "  Na(k) +          H2O    →      Na+(aq)      +     OH-(aq)     +      1/2H2(g)  BF3 +          F-      →        BF4-       3. PbO       +        SO3      →      PbSO4

50.00 mL of a buffer solution contains 0.280 M HClO and 0.450 M NaClO.  If 25.00 mL of water is added to the buffer, what are the new concentrations of HClO and NaClO?

1. Students were responsible for conducting 3 trials of titration of 10 mL samples of phosphoric acid, H3PO4, with volumes of a 2.0 molar (mol/L) sodium hydroxide, NaOH, solution. What is the concentration of the phosphoric acid solution using the results that were obtained? K Given: H₂PO4(aq) + 3NaOH(aq) - Na3PO4(aq) + 3H₂O(1) Initial Buret Reading (mL) Final Buret Reading (mL) Volume Base Added (mL) 2 => Na Mg Rb Sr 2.92 M Cs Ba 0.55 M 1.21 M Be 0.97 M 1.76 M Ca Sc 3.11 M Ra La 91 AM Hf Ac Trial 1 0.3 14.2 TI Zr Nb Mo Tc [81 $4 Cr Mn Fe Re Os Rf Db Sg Bh Hs Periodic Table of the Elements T Trial 2 14.2 A Basic D 30.0 Symbol 10 77 78 224, Co Ni Cu Zn Ga B 14 Neble Gas Trial 3 30.0 43.9 Ru Rh Pd Ag Cd In Sn Sb Te M с N Expe 201 VIA Sm Nd Pm Eu Gd Dy Ho "Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 15 VIA M He Ge As Se Br Kr Xe Pt Au Hg Ds Rg Cn Uut FI Uup Lv Uus Uuo Ne "Er Tm Yb

Acetic acid (CH3COOH) is a product of many microbial metabolisms. It forms acetate ion and a hydrogen ion according to the folllowing reaction: CH3COOH(aq) ↔ CH3COO(aq) - + H + K = 2.0 x 10^-5 I'm a total granola type who makes his own vinegar at home. (Vinegar is acetic acid.) I measured the pH of the vinegar I made to be 2.7. (Recall, pH = -log10[H+]). What is the molar concentration of acetic acid in my vinegar, to two decimal places

What is the pH of the solution that results from adding 25.0 mL of 0.012 M NaOH to 25.0 mL of 0.024 M lactic acid, C3H5O3H? C3H5O3H(aq) + OH-(aq) → H2O(ℓ) + C3H5O3-(aq) Ka for lactic acid = 1.4×10-4 pH =

Complete the balanced molecular reaction for the following weak acid with a strong base: HNO2(aq) + Ca(OH)2(aq) ->