How many mL of 0.115 M NaOH will react with exactly with 22 mL of a 0.210 M solution of H2SO4 (3 SF) 2 NaOH (aq) + H2SO4 (aq) --> Na2SO4 (aq) + 2 H2O (l)

2AgNO3(aq) +CaBr2(aq) --> 2AgBr(s) + Ca(NO3)2 (aq). Calculate the excess of the excess reagent, in moles, when 25mL of .300 M AgNO3 is added to 25.0 mL of .250 M CaBr2

What weight of potassium hydrogen phthalate will require 30. mL of a 0.30M NaOH solution to reach the equivalence point? KHP MM 204.22 g/mol .CO;K' .CO;K' NaOH + H2O + *CO,H COƠ,Na'

Determine the number of grams of PbCl2 produced from 100.0 ml of 0.20 M Pb(NO3)2 and sufficient NaCl in the following precipitate reaction  2 NaCl + Pb(NO3)2 --> PbCl2 + 2 Na(NO3)   Could you please solve by filling in the blanks in the image.

55.0 mL of 1.20 M H2SO4 is added to a 39.5 mL of 2.00 M LiOH. The balanced chemical equation for the reaction is: H2SO4 (aq) + 2LiOH (aq) --> Li2SO4 (aq) + 2H2O (l)  What kind of reaction is this? If a phenolphthalein indicator was included in the reaction flask, what color will it be after the 55.0 mL of 1.20 M H2SO4 and 39.5 mL of 2.00 M LiOH have reacted? Clear or pink? Explain your answer and include any relevant calculations.

10. If 29.50 mL of 0.175 M nitrous acid neutralizes 50.0 ml. of harium hydroxide, what is the molarity of the base? 2HNO;(aq) + Ba(OH);(aq) Ba(NO:)(aq) + 2H;O(1)

Use the equation below to calculate the following: 2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) (d) the grams of Na2SO4 that can be obtained from 27 mL of 0.075 M NaOH (e) the volume of 0.344 M H2SO4 needed to react with 29.3 mL of 0.827 M NaOH (f) the molarity (M) of the NaOH solution when 51.71 mL react with 64.50 mL of 0.171 M H2SO4

6. How many milliliters of 0.175 M Hg(NO3)2 is needed to completely precipitate 2.50 g KI? (Molar mass of KI = 166.0 g/mol) %3D Hg(NO3)2(aq) + 2 KI(aq) 2 KNO3(aq) + Hgl2(s)

Calculate the molarity of a Fe2+ (aq) solution given that a 25.00 mL sample of that solution requires 6.80mL of a 0.0653M solution of Ce4+ (aq).  Fe2+(aq) + Ce4+(aq) --> Fe3+(aq) + Ce3+(aq) a. 0.0356M b. 0.0178M  c. 8.88 x 10-3 M d. 1.11 x 10-5 M e. 3.56 M

You prepare a standard NaOH solution 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. It took 31.55 mL of the NaOH solution to titrate (react exactly with) 0.750 g KHP. You then use the standard base solution to determine the amount of ascorbic acid in a 500.0 mg tablet of vitamin C. Ascorbic acid (HC₆H₇O₆, molar mass 176.12 g/mol) also has one acidic hydrogen, and is usually mixed with some filler in preparing the tablets. It requires 17.54 mL of the NaOH to titrate (react exactly with) the ascorbic acid found in one 500.0 mg tablet. What is the percent vitamin C by mass in the tablet?