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What volume in mL of a 1.06 M NaOH solution is required to neutralize 11 g of HCl?
Balanced equation. NaOH + HCl -> NaCl + H2O all one to one. find moles HCl. 11 grams HCl (1 mole HCl/36.458 grams ) = 0.3017 moles HCl Moles HCl same as moles NaOH Molarity = moles of solute/Liters of solution 1.06 M NaOH = 0.3017 moles NaOH/liters of solution = 0.2846 Liters this is equal to..... 285 milliliters of NaOH needed
How many moles of NaOH will it take to neutralize 0.61 L of 0.46 M HCl?
1st Get the balanced equation NaOH + HCl -> NaCl + H2O Find the number of moles in HCl; n = cv n = 0.46x0.61 n = 0.2806 moles the number of moles of HCl and NaOH is the same so 0.2806moles will be needed
What is the minimum molarity of HCl when titrated with 18.6ml of NaOH?
First of all, it is HCl solution, more properly hydrochloric acid (that is HC l ). It is composed of hydrogen (H) and chlorine (Cl). The answer depends on the volume of the acid and the concentration of the alkali. Here is a sample calculation with some random values for the variables you have not given. If the HCl is neutralized by 25.0 ml of 0.500 M NaOH, then the number of moles of NaOH equals the number of moles of HCl. 25 ml is equal to 0.025 liters, and since molarity is moles per liter we have: Moles of NaOH = 0.0250 Liters * 0.500 moles/liter = 0.0125 moles Moles of NaOH = moles of HCl = 0.0125 moles If there are 0.0125 moles HCl in 45.0 ml (or 0.045 L), then the molarity of the HCl is: 0.0125 moles ÷ 0.0450 L = 0.278 moles/L = 0.278 M HCl
How do you test hydrochloric acid whether it is strong or weak?
What you are doing here is titration. You know you have a solution of HCl, but you do not know how much HCl is in it. For this you use something that can react with HCl (NaOH) and use an indicator to tell you when the reaction is complete. The reaction is pretty simple: HCl + NaOH --> H2O + NaCl You can see here that NaOH and HCl have a 1:1 mol relationship. So, lets find out how many moles of NaOH you used up with concentration = moles/volume 0.10 M NaOH = moles NaOH/ 0.0197 L NaOH solution Remember that M is in moles/L moles NaOH = 0.00197 moles Since you have a 1:1 relationship of NaOH with HCl, the 0.00197 mol applies to HCl as well. The next question works the same way, but backwards. Try doing it yourself if you understood the first part before reading my answer. Find out how many moles of HCl you have so you can find out how much moles of NaOH you need for the neutralization. 0.050 M HCl = n HCl / 0.020 L HCl soln n HCl = 0.001 mol HCl Remeber the 1:1 relationship, which gives you that n NaOH = 0.001 mol. Now all you need is the volume. 0.1 M NaOH = 0.001 mol NaOH/ Volume soln V = 0.01 L = 10 mL
How many Moles of Na react with how many Moles of Cl?
Balanced equation first. NaOH + HCl >> NaCl + H2O Everything is one to one, so 1.222 moles HCl (1mole NaOH/1mole HCl) = 1.222 moles NaOH
What volume in mL of a 1.06 M NaOH solution is required to neutralize 11 g of HCl?
Balanced equation. NaOH + HCl -> NaCl + H2O all one to one. find moles HCl. 11 grams HCl (1 mole HCl/36.458 grams ) = 0.3017 moles HCl Moles HCl same as moles NaOH Molarity = moles of solute/Liters of solution 1.06 M NaOH = 0.3017 moles NaOH/liters of solution = 0.2846 Liters this is equal to..... 285 milliliters of NaOH needed
How many moles of NaOH will it take to neutralize 0.61 L of 0.46 M HCl?
1st Get the balanced equation NaOH + HCl -> NaCl + H2O Find the number of moles in HCl; n = cv n = 0.46x0.61 n = 0.2806 moles the number of moles of HCl and NaOH is the same so 0.2806moles will be needed
How many moles of NaCl are formed from the reaction between 1.4 moles of HCl and 2.8 moles NaOH?
1.4 moles - the HCl is the limiting ingredient
What is the minimum molarity of HCl when titrated with 18.6ml of NaOH?
First of all, it is HCl solution, more properly hydrochloric acid (that is HC l ). It is composed of hydrogen (H) and chlorine (Cl). The answer depends on the volume of the acid and the concentration of the alkali. Here is a sample calculation with some random values for the variables you have not given. If the HCl is neutralized by 25.0 ml of 0.500 M NaOH, then the number of moles of NaOH equals the number of moles of HCl. 25 ml is equal to 0.025 liters, and since molarity is moles per liter we have: Moles of NaOH = 0.0250 Liters * 0.500 moles/liter = 0.0125 moles Moles of NaOH = moles of HCl = 0.0125 moles If there are 0.0125 moles HCl in 45.0 ml (or 0.045 L), then the molarity of the HCl is: 0.0125 moles ÷ 0.0450 L = 0.278 moles/L = 0.278 M HCl
How do you test hydrochloric acid whether it is strong or weak?
What you are doing here is titration. You know you have a solution of HCl, but you do not know how much HCl is in it. For this you use something that can react with HCl (NaOH) and use an indicator to tell you when the reaction is complete. The reaction is pretty simple: HCl + NaOH --> H2O + NaCl You can see here that NaOH and HCl have a 1:1 mol relationship. So, lets find out how many moles of NaOH you used up with concentration = moles/volume 0.10 M NaOH = moles NaOH/ 0.0197 L NaOH solution Remember that M is in moles/L moles NaOH = 0.00197 moles Since you have a 1:1 relationship of NaOH with HCl, the 0.00197 mol applies to HCl as well. The next question works the same way, but backwards. Try doing it yourself if you understood the first part before reading my answer. Find out how many moles of HCl you have so you can find out how much moles of NaOH you need for the neutralization. 0.050 M HCl = n HCl / 0.020 L HCl soln n HCl = 0.001 mol HCl Remeber the 1:1 relationship, which gives you that n NaOH = 0.001 mol. Now all you need is the volume. 0.1 M NaOH = 0.001 mol NaOH/ Volume soln V = 0.01 L = 10 mL
What is the limiting reagent in a reaction?
The limiting reagent in a reaction is the reactant that runs out first. For example, if you are reacting 10 moles of HCl and 5 moles of NaOH, you will get 5 moles of H20, 5 moles of NaCl, and 5 moles of HCl, because the remaining HCl had nothing to react with. Therefore, the NaOH is the limiting reagent.
How many Moles of Na react with how many Moles of Cl?
Balanced equation first. NaOH + HCl >> NaCl + H2O Everything is one to one, so 1.222 moles HCl (1mole NaOH/1mole HCl) = 1.222 moles NaOH
How many moles of HCl are required to completely react with .005 moles of NaOH?
Simple equality. (X L)(2.5 M HCl) = (1.5 L)(5.0 M NaOH) 2.5X = 7.5 X = 3.0 Liters needed ================
What happens when HCl is mixed with a solution that is not a buffer solution?
If the solution is not a buffer, the HCl will react with the solution to form a product.
What is the stoichiometric relationship between NaOH and HCl?
These chemicals react in a direct proportion of one to one, measured in moles of course, not by weight. A mole of NaOH weighs more than a mole of HCl.
How much caustic soda is required to neutralize a 25ml HCl solution at pH 3?
One step at a time.1/103 = 0.001 M HCl, so.....Molarity = moles of solute/Liters of solution ( 25 ml = 0.025 Liters )0.001 M HCl = X moles HCl/0.025 Liters= 2.5 X 10 - 5 moles HCl========================now, balanced eqiationNaOH + HCl --> NaCl + H2O ( all one to one )( now drive reaction towards mass NaOH )2.5 X 10 - 5 moles HCl (1 moles NaOH/1 mole HCl)(39.998 grams/1 mole NaOH)= 10 -4 grams caustic soda needed==========================
How many moles of HCL in 50ml of 1.0 M HCL?
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
