3. how would the following errors affect the concentration of Cl- obtained in question 2b? give your reasoning in each case. a. the student read the molarity of AgNo3 as 0.02104M instead of 0.02014M b. the student was past the endpoint of titration when he took the final buret reading.

4  A sample of solid Ca(OH)2 was stirred in water at a certain temperature until the solution contained as much dissolved Ca(OH)2 as it could hold. A 84.3-mL sample of this solution was withdrawn and titrated with 0.0771 M HBr. It required 86.7 mL of the acid solution for neutralization.  (a) What was the molarity of the Ca(OH)2 solution?  M    (b) What is the solubility of Ca(OH)2 in water, at the experimental temperature, in grams of Ca(OH)2 per 100 mL of solution?  g/100mL

What volume (in ml) of 0.12 M HBr solution is be required to titrate 125 mL of a 0.1 M Ca(OH)2 solution? Ca(OH)2(aq) + 2HBr(aq) ⟶ CaBr2(aq) + 2H2O(l)

a) Copper(I) ions in aqueous solution react with NH3(aq)NH3(aq) according to   Cu+(aq)+2NH3(aq)⟶Cu(NH3)+2(aq)?f=6.3×10^10 Calculate the solubility (in g·L−1) of CuBr(s)CuBr(s) (?sp=6.3×10−9Ksp=6.3×10−9) in 0.19 M0.19 M NH3(aq)NH3(aq). solubility of CuBr(s)CuBr(s): g/L b) Given the equation   Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)?f=2.00×107Ag+(aq)+2NH3(aq)⟶[Ag(NH3)2]+(aq)Kf=2.00×107   determine the concentration of NH3(aq) that is required to dissolve 589589 mg of AgCl(s) in 100.0 mL of solution. The ?spKsp of AgCl is 1.77×10−101.77×10−10. [NH3]=  c) The formation constant* of [M(CN)44]2− is 7.70×10167.70×1016, where M is a generic metal. A 0.1400.140 mole quantity of M(NO3)2 is added to a liter of 0.9700.970 M NaCN solution. What is the concentration of M2+ ions at equilibrium? [M2+]=

The active ingredient in a certain toilet cleaner that claims to ‘remove lime scale and rust’ is hydrochloric acid of approximate concentration 1.12 mol/L. To analyze this toilet cleaner, a quality control chemist first delivered a 16.2 mL aliquot of the toilet cleaner into a 250-mL volumetric flask, then made up the diluted solution. She then titrated a 24.8 mL aliquot of this diluted solution against standard sodium hydroxide solution of concentration 0.2178 mol/L. The expected titre (or volume of the titrant) would be approximately:

A student analyzed an antacid tablet from a bottle of 50 tables purchased at a discount store for $1.00. The mass of the tablet was 1.470 g.After adding 25.00 mL of 0.7989 M HCl solution to the tablet, the student back-titrated the excess HCl with 3.55 mL of 1.017 M NaOHsolution. Calculate the number of moles of stomach acid neutralized by one Calculate the mass effectiveness of the tablet (mol H+/g). Calculate the cost effectiveness of one tablet ($/mol H+).

A 0.411 g sample of potassium hydrogen phthalate, KHC8H4O4 (molar mass = 204.22g/mol), is dissolved with 50.0 mL of deionized water in a 125mL Erlenmeyer flask. The sample is titrated to the phenolphthalein endpoint with 15.17 mL of a sodium hydroxide solution. What is the molar concentration of the NaOH solution? Express the molar concentration of NaOH to the correct number of significant figures.

Consider the titration of H2SO4 with NaOH. A 30.0 L sample of H2SO4 requires 0.090L of 0.100 M NaOH. What are the moles ofacid? Number of molecules of the acid? Molarity of Acid? what is the grams of Acid present?A. Moles of Acid?B. Molecules of AcidC. Molarity of AcidD. grams of Acid?

What volume of 0,955 mol·dm–3 HCl solution (in mL or cm3), is required to titrate 2,152 g of Na2CO3 to the equivalence point? The reaction is: Na2CO3 (aq)+2HCl(aq)→H2O(l)+CO2 (g)+NaCl(aq)