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- A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol blue endpoint using 19.8 mL of 0.0998M NaOH. How many moles and how many grams of the base are in the antacid sample? Assume the active ingredient is MgCO3. Moles of NaOH? Moles of HCl? Moles of MgCO3? Mass of MgCO3?calculate molarity of acetic acid in vinegar: (volume of NaOH 3ml, cincentration of NaOH 24.215, titrate average use of NaOH 3.44mL). then convert your M concentration of acetic acid to %w/w, given the density of vinegar is 1.005 g/mL.What is [H3O+ ] (in M) in a solution of 0.063 M HCNO and 0.035 M NaCNO? (Assume Kw = 1.01 ✕ 10−14.) HCNO(aq) + H2O(l) H3O+(aq) + CNO−(aq) Ka = 3.5 ✕ 10−4
- What amount of solid NaOH must be added to 1.0 L of a 0.10 MH2CO3 solution to produce a solution with [H+] = 3.2 * 10-11 M?There is no significant volume change as the result of adding thesolid.Hydroiodic acid often is used to disinfect and sanitize medical tools and products. In an experiment, 5.0 mL of 0.75 mol/L HI(aq) is mixed with 20.0 mL of distilled water. (record only your final answer with the correct number of significant digits and the proper units.) 1. What is the hydronium ion concentration of the resulting diluted solution? 2. What is the pH of the resulting solution? 3. If 1.0 mL of the diluted solution is added to 9.0 mL of distilled water, what is the resulting pH of the solution? 4. If 1.0 mL of the diluted solution from #3 is added to 9.0 mL of distilled water, you should be able to predict the pH based on the trend you see and without doing any calculations. This is because every time the hydronium concentration a) increases b)decreases by a factor of 10, the pH goes up one full unit since the solution becomes a)more b)less acidic.Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 1.5 × 10−6) is titrated with 0.10 M NaOH solution. The ionization of HA in water occurs as the following.HA (aq) + H2O(l) ⇌ A-(aq) + H3O+ (aq)The neutralization reaction between HA and NaOH can be expressed as the following. HA (aq) + NaOH (aq) ® NaA (aq) + H2O (l) Answer the following questions. A) What will be the initial pH of the 0.10 M HA solution?
- The concentration of hydrogen peroxide H202) solutions can be determined by titrating with HI according to the balanced chemical eauation below. If 35.2 mL of 1.5 M HI solution was required to titrate 135.2 mL of a H20, solution what is the molarity of the H20, solution? 2 HI(aq) + H202(aq)-> I2(aq) + H2O(l)A 0.7500 g sample of a phosphoric acid (H3PO4) solution with unknown concentration requires 30.00 mL of 0.3375 M NaOH to reach the end point. Calculate the %(m/m) concentration of the phosphoric acid in the unknown solution. H3PO4(aq) + 3NaOH(aq)---> K3PO4(aq) + 3H2O(l)Write the products for the balanced equation for the dissociation into ions of each of the following soluble salts in aqueous solutions: Input the cation and then anion with correct coeffiecients and charges. For example: The answer for ??(??3)2⟶??2++2??−3Ba(NO3)2⟶Ba2++2NO3− would be inputted in two separate fields, inputting the cation first: Ba^2+ 2NO_3^- Use carats for superscripts and underscores for subscripts. Include coefficients, if the coefficient is greater than 1. a) ???⟶CaS⟶ + b) ??3??4⟶Na3PO4⟶ +
- 0.4723-g sample of primary-standard-grade Na2CO3 required 34.78 mL of an H2SO4 solution to reach the end point in the reaction below. What is the molar concentration of the H2SO4?A solution of HCl with a volume of 25.00 mL is titrated to the endpoint, with 0.250 M NaOH. If it takes 34.56 mL of NaOH, what is the original concentration of HCl in the solution?: HCl (aq) + NaOH (aq) ---> H20 (l) + NaCl (aq)A 20.0 mL sample of vinegar is titrated with 0.108 M NaOH in the presence ofphenolphthalein indicator. If the vinegar requires 39.1 mL of NaOH solution for the completereaction, what is the concentration of acetic acid HC2H3O2 in the vinegar? The reaction is HC2H3O2(aq) + NaOH(aq) → NaC2H3O2(aq) + H2O(l)