A buffer solution that is 0.403 M in HF and 0.403 M in NaF has a...

A buffer solution that is 0.403 M in HF and 0.403 M in NaF has a pH of 3.14.

(1) The addition of 0.01 mol of H₃O⁺ to 1.0 L of this buffer would cause the pH to _________increase slightly increase by 2 units decrease slightly decrease by 2 units not change.

(2) The capacity of this buffer for added H₃O⁺could be increased by the addition of 0.148 mol_________of the weak acid of the salt.

Consider these compounds:

A. CaCrO₄

B. Fe₂S₃

C. CaCO₃

D. Ca₃(PO₄)₂

Complete the following statements by entering the letter corresponding to the correct compound.

Without doing any calculations it is possible to determine that zinc phosphate is more soluble than , and zinc phosphate is less soluble than .

It is not possible to determine whether zinc phosphate is more or less soluble than by simply comparing K_sp values.

Please show your work and be specific, I have asked these questions already and got the wrong answers because they weren't answered fully!

Expert Solution

queen_honey_blossom answered 2 years ago

A 360.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A)...

A 360.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A) What mass of NaOH could this buffer neutralize before the pH rises above 4.00? B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00? I keep getting 1.8 g and 3.5 g, which is wrong.

A 340.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. Part...

A 340.0 −mL buffer solution is 0.170 M in HF and 0.170 M in NaF. Part A What mass of NaOH could this buffer neutralize before the pH rises above 4.00? Express your answer using two significant figures. m = g Part B If the same volume of the buffer was 0.350 M in HF and 0.350 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00? Express your answer using two significant figures.

A 360.0 −mL buffer solution is 0.160 M in HF and 0.160 M in NaF. What...

A 360.0 −mL buffer solution is 0.160 M in HF and 0.160 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?

A 360.0 −mL buffer solution is 0.130 M in HF and 0.130 M in NaF. Part...

A 360.0 −mL buffer solution is 0.130 M in HF and 0.130 M in NaF. Part A) What mass of NaOH can this buffer neutralize before the pH rises above 4.00? Part B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?

#16.51 A 340.0 −mL buffer solution is 0.130 M in HF and 0.130 M in NaF....

#16.51 A 340.0 −mL buffer solution is 0.130 M in HF and 0.130 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? ANSWER: 0.98 If the same volume of the buffer was 0.340 M in HF and 0.340 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00?

A 340.0 −mL buffer solution is 0.140 M in HF and 0.140 M in NaF. What...

A 340.0 −mL buffer solution is 0.140 M in HF and 0.140 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? And, If the same volume of the buffer was 0.370 M in HF and 0.370 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00? Please show all steps. Thank you

A 25.0 mL buffer solution is 0.350 M in HF and 0.150 M in NaF. Calculate...

A 25.0 mL buffer solution is 0.350 M in HF and 0.150 M in NaF. Calculate the pH of the solution after the addition of 37.5 mL of .200 M HCl. The pKa for HF is 3.46.

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate...

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.

A 350 mL buffer solution containing 0.15 M HF and 0.150 M NaF is reacted with...

A 350 mL buffer solution containing 0.15 M HF and 0.150 M NaF is reacted with sodium hydroxide. What mass of NaOH can this buffer neutralize before the pH rises above 4.0? If the same volume of buffer was 0.35 M in HF and 0.35 M in NaF then what mass of NaOH could be handled before the pH rises above 4.0?

A 1.0 L buffer solution is made up of 0.15M NaF and 0.20 M HF (...

A 1.0 L buffer solution is made up of 0.15M NaF and 0.20 M HF ( pK a = 3.17) . 0.05 mol of HCl is added to it. What is the new pH?

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