We know that,
For neutralization reaction,
Number of moles of acid= Number of moles of base
i.e.
n(base) = n(acid)
n(NaOH) = MV/1000
n(NaOH) = 0.250×50.0/1000
n(NaOH) = 0.0125 moles
help with #1 please 1) How many moles of NaOH would you need to neutralize 50.0...
How many grams of sodium hydroxide (NaOH) would be needed to neutralize 50.0 mL of 0.500 M phosphoric acid (H_3 PO_4)? H_3 PO_4 + NaOH rightarrow Na_3 PO_4 + HOH (unbalanced)
How many mL of 1.000M NaOH solution would it take to neutralize 10.0mL of vinegar that contained 0.500M acetic acid? 5.50mL 4.50mL 5.40mL 5.00mL D Question 4 2 pts If 20.00 mL of a 0.1000M solution of NaOH is required to neutralize 10.00mL of vinegar, then the molarity of the acetic acid is 0.2500M 0.2000 M 0.5000 M Question 1 2 pts There is a 3:1 ratio between NaOH and acetic acid in the balanced chemical equation for this lab....
What is a polyprotic acid? 2. How many moles of H3O + are present in 50 mL of 0.3 M H2SO4? 4. If 20.20 mL of 0.122 M NaOH are required to reach the first equivalence point of a solution of citric acid (H3C6H5O7), how many mL of NaOH are required to completely neutralize this solution? 5. If the pH at one-half of the neutralization points of a dibasic acid is 3.52 and 6.31 respectively, what are the values for...
need help with number 2 please
When the formation of a salt of a strong Strong Acid 2. What is the pH of the solution obtained by mixing 50.00 mL of 0.250M HCl and 50.00 mL of 0.500M NaOH HCl + Naot & H₂O Strong base I 12.5 25. - 12.5 = 12.5 mmol HCl - 25ml NaOH
help please
Consider a titration of 0.0200 moles HCl (a strong acid) with NaOH (a strong base). At the equivalence point, the total volume of the solution is 78.9 mL. What is the pH of this solution at this equivalence point?
1- A) How many milliliters of 0.100 M NaOH are needed to neutralize 50.00 mL of a 0.150 M solution of acetic acid (CH3COOH), a monoprotic acid? View Available Hint(s) B)What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH solution for neutralization? C))What is the concentration of a phosphoric acid solution of a 25.00 mL sample if the acid requires 42.24 mL of 0.135 M...
I need help with this please. 1. Calculate the volume of a 0.1M NaOH that 40.0 ml of the buffer could neutralize ( the pH of the buffer is 4.9) 2. Calculate the volume of a 0.1M HCl that 40.0 ml of the buffer could neutralize ( the pH of the buffer is 4.9) 3. How would your answers to 1 and 2 change if the system was made starting with 100.00ml of 0.010 M sodium acetate. The buffer is...
1. How many mL of 0.100 M NaOH are required to neutralize (or titrate) 25.0 mL of 0.15 M H,Po.? Write the balanced acid-base neutralization reaction to start. (12 pts)
1. Calculate the volume (in mL) of the amount of 0.200 M NaOH required to neutralize a monoprotic weak acid solution made by 2.00 g of potassium hydrogen phthalate (KHP) dissolved in water. Hint: the complete neutralization occurs at the equivalence point, where the number of moles of the analyte (in this case, the weak acid) equal to the titrant (in this case, the strong base). 2. Identify the equivalence point, the half-equivalence point on the titration curve below and...
50.0 mL sample of the weak acid
the concentration of the weak acid = 0.15 M
25 mL of the week acid into 100 mL beaker
titrated this solution of 0.21 M NaOH
moles of weak acid = 3.75*10^-3
moles of NaOH = moles of week acid
c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...