A)
Balanced chemical equation is:
HCl + NaOH ---> NaCl + H2O
Here:
M(HCl)=0.2099 M
V(HCl)=8.97 mL
V(NaOH)=8.0 mL
According to balanced reaction:
1*number of mol of HCl =1*number of mol of NaOH
1*M(HCl)*V(HCl) =1*M(NaOH)*V(NaOH)
1*0.2099*8.97 = 1*M(NaOH)*8.0
M(NaOH) = 0.2354 M
Answer: 0.235 M
B)
Balanced chemical equation is:
HCl + NaOH ---> NaCl + H2O
Here:
M(HCl)=0.1061 M
V(HCl)=11.14 mL
V(NaOH)=21.0 mL
According to balanced reaction:
1*number of mol of HCl =1*number of mol of NaOH
1*M(HCl)*V(HCl) =1*M(NaOH)*V(NaOH)
1*0.1061*11.14 = 1*M(NaOH)*21.0
M(NaOH) = 0.05628 M
Answer: 0.05628 M
C)
Balanced chemical equation is:
HCl + NaOH ---> NaCl + H2O
Here:
M(HCl)=0.0889 M
V(HCl)=10.85 mL
V(NaOH)=12.0 mL
According to balanced reaction:
1*number of mol of HCl =1*number of mol of NaOH
1*M(HCl)*V(HCl) =1*M(NaOH)*V(NaOH)
1*0.0889*10.85 = 1*M(NaOH)*12.0
M(NaOH) = 0.0804 M
Answer: 0.0804 M
Exercise 14.48- Enhanced - with Feedback Four solutions of unknown NAOH concentration are titrated with...
Exercise 14.47 Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution Part A Calculate the concentration (in M) of the unknown HCl solution in the first case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 20.00 mL 27.44 mL 0.1191 M HCI Volume (mL) 20.00 mL 14.00 mL...
Exercise 14.47 Review Part Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Calculate the concentration (in M) of the unknown HCl solution in the third case. HCI Volume (ml) NaOH Volume (mL) (NaOH (M) 24.00 mL 13.88 mL 0.1178 M Express your answer using four significant figures....
Four solutions of unknown NaOH concentration are titrated with solutions of HCl. The following table lists the volume of each unknown NaOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. NaOH Volume (mL) HCl Volume (mL) [HCl] (M) 7.00 mL 9.17 mL 0.2099 M 18.00 mL 10.84 mL 0.1111 M 15.00 mL 10.75 mL 0.0489 M 26.00 mL 35.18 mL 0.1421 M Part A: Calculate the concentration (in M)...
Four solutions of unknown HCl concentration are titrated with solutions of NaOH. The following table lists the volume of each unknown HCI solution, the volume of NaOH solution required to reach the equivalence point, and the concentration of each NaOH solution. Part BCalculate the concentration (in M) of the unknown HCl solution in the second case.
Part A The titration of 23.40 mL of HCl solution of unknown concentration requires 12.18 mL of a 0.140 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M? Express your answer in moles per liter to three significant figures. We ΑΣΦ ? M(HCI) M Submit Request Answer
Titrations 1. A 50.00-ml NaOH sample of unknown concentration was titrated with 0.1274 M HCI. if 33.61 mL of the HCl solution were required to neutralize the NaOH sample, what is the molarity of the NaOH sample? Show the steps in your calculation 2. A 25.00-ml HCl sample of unknown concentration was titrated with 0.5631 M Al(OH)3. If 37.62 mL of the Al(OH) solution were required to neutralize the HCl sample, what is the molarity of the HCl sample? (Assume Al(OH)3 is...
The titration of 23.30 mL of HCl solution of unknown concentration requires 13.00 mL of a 0.200 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution in M? Express your answer in moles per liter to three significant figures. M(HCl)M(HCl) = _____________
A 25.0 mL NaOH solution of unknown concentration was titrated with a 0.189 M HCl solution. 19.6 mL HCl was required to reach equivalence point. In a separate titration, a 10.0 mL H3PO4 solution was titrated with the same NaOH solution. This time, 34.9 mL NaOH was required to reach the equivalence point. What is the concentration of the H3PO4 solution?
Exercise 14.50 - Enhanced - with Feedback A 5.30 mL sample of an H3PO4 solution of unknown concentration is titrated with a 1.050~10-2 M NaOH solution. A volume of 7.22 mL of the NaOH solution was required to reach the equivalence point. Part A What is the concentration of the unknown H3PO4 solution? You may want to reference (Pages 494 - 497) Section 14.6 while completing this problem. Express your answer with the appropriate units. ? CH Å Value M...
Suppose that 10.00 mL HCl of unknown concentration is neutralized by 20.00 mL of a 1.50 M NaOH solution. Determine the concentration of the HCl solution 1.50 M HCI 3.00 M HCI 0.0750 M HCI 0.150 M HCI