A Carbon dioxide dissolves in water to produce carbonic acid (H;co,). Under normal atmospheric conditions, the total amount of carbonic acid (in all forms) in water is 1.2 x 10* M. Which is the correct mass balance equation for carbonate? Equation 1: [H;CO3] = [HC05] + [co5²] Equation 2: [H*] = [OH-]+ [HCO5]+ 2 × [[co5*] 1.2 x 10 -8 = [H;CO3] + [HCO5]+ [CO5²] 1.2 x 10-8 = [OH-]+ [HCO5]+ 2 × [co5] Equation 5: 1.2 x 10 -º = [H2CO3] + [HCO5]+ 2 × [co5ª] Equation 3: Equation 4: B What is the predominant form of the triprotic acid, citric acid, at pH 6.2? Answer options: H,A, H;A', HA*?, A Calculate oma and la. for acetic acid in a solution that has a pH of 5.32. Answer options: 0.05 and 0.95; 0.21 and 0.79; 0.56 and 0.44; 0.72 and 0.28

Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. NH3(aq) + HCl(aq) – ->

An analytical chemist weighs out 0.318 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 82.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol x10 x 3

You are performing an experiment in lab that involves the titration of a H2SO4 solution. You titrate the acidic solution with 0.5166 M NaOH and the equivalence point is reached by the addition of 21.76 mL of NaOH solution. Using the balanced equation below, calculate the moles of H2SO4 in the flask. Do NOT include units or write the answer in scientific notation. 2NaOH(aq) + H2SO4(aq) → 2H2O(l) + Na2SO4(aq)

A chemistry student weighs out 0.0856 g of citric acid (H,CH,0,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0900 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL x10

A)When working in the lab, you are measuring the pH of a system. The pH meter reads 4.34. What is the concentration of [H3O+] in solution? B)You have created a solution of NaOH by dissolving NaOH in water. You determine that the [OH-] concentration in solution is 4.37 x 10-9. What is the pOH of the solution? C)What is the pH of a solution containing an [H3O+] = 9.67 x 10-3?

You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?

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Ammonia and sulfuric acid reacts according to the equation given below. how many. Military of 0.110 M sulfuric acid are required to exactly neutralize 25.0 mL of 0.0840 M NH_3 solution:2NH_3 (aq)——> (NH_4)_2 SO_4(aq)

Part A Calculate the concentrations of K+ and F in a 0.19 M KF solution. Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by a comma. [K], [F]=0.19,0.19 M Submit Previous Answers Part B Correct As a soluble ionic compound, KF undergoes complete dissociation in an aqueous solution: KF (aq) →K+ (aq) + F-(aq) To a first approximation, you can ignore the basic properties of the anion since the concentration of hydroxide ion is significantly lower than the concentrations of K+ and F. Therefore, [K+] = [F]= 0.19 M. Calculate the concentrations of HF, OH, and H3O+ in a 0.19 M KF solution (for which Ka (HF) = 6.8 × 10-4). Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by commas. ΜΕ ΑΣΦ [HF], [OH], [H3O+] = ? M