1. if 15.0mL of 4.5 M NaOH are diluted with water to a volume of 500mL, what is the molarity of the resulting solution?

2. in a acid-base titration, 33.65mL of an 0.148 M HCL solution were required to neutralize 25.00mL of a NaOH solution. What is the molarity of the NaOH solution?

3. a 0.481 gram sample of an unknown acid (HX) required 28.95 mL of 0.2103 M NaOH for neutralization to a phenolphthalein endpoit. What is the molar mass of the acid?

4. what volume of 0.1037 M HCL is necessary to neutralize 0.3643 grams Ca(OH)2? included a balanced equation?

5.calculate the molar concentration of propionic acid (HC3H5O2) in solution if 10.00mL of a propionic acid solution is neutralized with 16.85mL of 0.143 M NaOH solution.

6. calculate the mass percent of propionic acid (HC3H5O2) in solution. (Assume the density of the solution to be 1.00g/mL.)

You fare better if you post one question per try.

1.
M1 x mL1 = M2 x mL2

2.
Since NaOH and HCl react 1:1 (write the balanced equation to see that), then
mLHCl x MHCl = mLNaOH x M NaOH

3.
moles NaOH = M x L = ?
moles HX = the same
moles HX = grams/molar mass
Solve for molar mass.

which of the following Al acid ?(1)s2- (ii)H3O+ (iii)NO3- (iv)k+

What is the concentration of NaOH if 5mL of 5.0 N is diluted to 500mL?

1. To find the molarity of the resulting solution, you need to use the formula: M1V1 = M2V2, where M1 is the initial molarity, V1 is the initial volume, M2 is the final molarity, and V2 is the final volume. In this case, M1 is 4.5 M, V1 is 15.0 mL, and V2 is 500 mL. You want to find M2, so rearrange the formula to solve for M2: M2 = (M1 * V1) / V2. Plug in the values to get M2 = (4.5 M * 15.0 mL) / 500 mL. Calculate this to get the final molarity.

2. In an acid-base titration, you need to use the concept of stoichiometry to find the molarity of the NaOH solution. For this, you need to establish a balanced equation representing the reaction that occurs between HCl and NaOH. The balanced equation is: HCl + NaOH -> NaCl + H2O. From the equation, you can see that one mole of HCl reacts with one mole of NaOH. Using the molar ratio, you can calculate the moles of HCl used in the titration by multiplying the volume of HCl solution (33.65 mL) by its molarity (0.148 M). Next, divide the moles of HCl by the volume of NaOH solution (25.00 mL) to get the molarity of the NaOH solution.

3. To find the molar mass of the acid (HX), you need to use the concept of stoichiometry and the definition of molarity. From the balanced equation involved in the neutralization reaction, you can determine that one mole of NaOH reacts with one mole of HX. Use the volume of NaOH solution (28.95 mL) and its molarity (0.2103 M) to calculate the number of moles of NaOH used in the reaction. Then, using the molar ratio from the balanced equation, determine the number of moles of HX. Finally, divide the mass of the acid (0.481 grams) by the moles of HX to find the molar mass.

4. The balanced equation for the neutralization reaction between HCl and Ca(OH)2 is: 2 HCl + Ca(OH)2 -> CaCl2 + 2 H2O. From the equation, you can determine that each mole of Ca(OH)2 reacts with two moles of HCl. To find the volume of HCl needed, start by finding the number of moles of Ca(OH)2 using its molar mass. Then, use the molar ratio to determine the moles of HCl required. Finally, divide the moles of HCl by its molarity to find the volume in liters.

5. To calculate the molar concentration of propionic acid (HC3H5O2), you need to use the neutralization reaction with NaOH. First, write a balanced equation for the reaction: HC3H5O2 + NaOH -> NaC3H5O2 + H2O. From the equation, you can determine that one mole of HC3H5O2 reacts with one mole of NaOH. Using the volume of NaOH solution (16.85 mL) and its molarity (0.143 M), you can calculate the number of moles of NaOH used in the neutralization. Then, using the molar ratio from the balanced equation, determine the number of moles of HC3H5O2. Finally, divide the moles of HC3H5O2 by the volume of the propionic acid solution (10.00 mL) to find its molar concentration.

6. To calculate the mass percent of propionic acid (HC3H5O2) in solution, you need to divide the mass of the acid by the mass of the solution and multiply by 100%. First, find the mass of propionic acid by multiplying its molar mass by the number of moles calculated in a similar manner as in question 5. Then, find the mass of the solution by multiplying its density by its volume. Finally, divide the mass of the propionic acid by the mass of the solution and multiply by 100% to get the mass percent.